Which Of The Following Is Consistent With The Law Of Supply?

Which Of The Following Is Consistent With The Law Of Supply
Answer: d. An increase in market price will lead to an increase in quantity supplied. When all else is constant, the law of supply states that the price and the quantity supplied have a direct relationship. If the market price of the output increases, the quantity supplied also increases.

Which of the following consistent with the law of demand?

Answer: The increase in the quantity of goods and services purchased due to a reduction in the market price is consistent with the law of demand.

Which statement is not consistent with the law of supply?

Which statement is not consistent with the law of supply? Quantity supplied of a good is inversely related to the good’s price. If supply and demand both shift to the right, equilibrium quantity: rises, but the equilibrium price may rise, fall, or stay the same.

What is an example of law of supply?

What Is a Good Example of the Law of Supply? – The law of supply summarizes the effect price changes have on a producer’s behavior. For example, a business will make more of a good (such as TVs or cars) if the price of that product increases. So, if the price of TVs increases, TV producers are incentivized to produce more of them.

Which of the following is the relation that the law of demand depends Mcq?

Law of demand is a fundamental principle of Economics, it states that quantity demanded is always inversely related to the price of the goods. Answer: b.

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Which of the following statement is inconsistent with Say’s law Mcq?

Which of the following statements is inconsistent with Say’s law? –

The economy has flexible wages and prices.
The economy will produce at the full-employment level of output.
The economy’s investment spending depends solely on the level of income.
The economy has an environment of “laissez faire.”

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Which of the following statements is the best statement for the law of supply?

Answer and Explanation: Option d. Price and quantity supplied are directly related, ceteris paribus. This option is correct because the law of supply states that there exists one to one relationship between price and quantity supplied.

Which of the following factors remain constant in the law of supply?

Assumptions to the law of supply: cost of all factors of production remains constant. The technology level remains constant.

What is called law of supply?

Suggest a new Definition Proposed definitions will be considered for inclusion in the Economictimes.com (##include msid=4006719,type=11 ##) Definition: Law of supply states that other factors remaining constant, price and quantity supplied of a good are directly related to each other. The above diagram shows the supply curve that is upward sloping (positive relation between the price and the quantity supplied). When the price of the good was at P3, suppliers were supplying Q3 quantity. As the price starts rising, the quantity supplied also starts rising. Snapshot: This is how the law of supply works.

What does the law of supply?

The law of supply is a fundamental concept in microeconomics that governs supply at a given price. The law of supply states that when the market price of a good increases, suppliers will increase the supply of that good. And when the price decreases, the quantity they will supply decreases.

What defines law of supply?

The law of supply states that a higher price leads to a higher quantity supplied and that a lower price leads to a lower quantity supplied. Supply curves and supply schedules are tools used to summarize the relationship between supply and price.

Which of the following are determinants of demand for a product or service Mcq?

Those determinants are: ​ Income of the buyer. Consumer trends and tastes. Expectations of future price, supply, needs, etc. The price of related goods.

Which of the following is correct expression of the first law of thermodynamics Mcq?

First law of thermodynamics MCQ – Objective Question Answer for First law of thermodynamics Quiz – Download Now! When a gas is compressed suddenly then its temperature

  1. Rises
  2. Decreases
  3. Remains unchanged
  4. None of the above

Let’s discuss the concepts related to and First law of thermodynamics. Explore more from here. Learn now! The correct answer is option 1) i.e. Raises, Key Points

  • An adiabatic process is where no heat is exchanged between the system and surroundings, This causes the compression of the gas.
  • There will be a change in the volume due to internal work done on the gas. So the work done is negative,
  • The first law of thermodynamics states that energy can neither be created nor destroyed.( ΔU = Q – W)
  • Energy can only be transferred or changed from one form to another.
  • ​For a system at thermodynamic equilibrium, the change in internal energy is equal to the difference in heat transfer of the system and work done on it.
  • Where ​ΔU is the change in internal energy, Q is the heat exchanged in the system and W is the work done during the thermodynamic process.

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students Which of the following statements is correct, in case of adiabatic expansion?

  1. ΔU = 0
  2. Δ U = negative
  3. Δ U = positive
  4. ΔW = 0

Concept:

  • The first law of thermodynamics states that the net heat energy supplied to the system is equal to the sum of the change in internal energy of the system and the work done by the system.
  • Adiabatic expansion is defined as the expansion in which there is no heat interaction of the system with the surroundings and work is done by the system at the expense of its internal energy.

Explanation:

  • In the case of adiabatic expansion, the volume of the system increases & hence work done is taken as positive but there is no heat exchange between the system & the surroundings which means that ΔQ = 0.
  • Therefore, From the first law of thermodynamics, we have
  • 0 = ΔU + W
  • ΔU = -W
  • ΔU = Negative Additional Information
  • In an isobaric process, the pressure of the system stays constant that is ΔP = 0, Thus the heat transferred to the system does work but also changes the internal energy of the system.
  • In an isochoric process, the volume of the closed system undergoing such a process remains constant that is ΔV = 0, Thus the heat transferred to the system changes the internal energy of the system.
  • In an isothermal process is a type of thermodynamic process in which the temperature T of a system remains constant that is ΔT = 0,

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students An ideal gas undergoes cyclic process ABCDA as shown in given P-V diagram (Fig.12.4). The amount of work done by the gas is

  1. 6P o V o
  2. -2P o V o
  3. +2P o V o
  4. +4P o V o
  1. CONCEPT:
  2. The amount of work done is wriiten as;
  3. \(\Delta W = PdV\)
  4. ⇒ \(\Delta W = P(V_f-V_i)\)
  5. Here P is the pressure and dV is the change in the volume.
  6. CALCULATION:
  7. Let us take the P-V diagram, in this figure we have work done in the process of ABCD is equal to the area of the rectangle in ABCDA.
  8. ⇒ work done in the process of ABCD = area of the rectangle in ABCDA.
  9. ⇒work done in the process of ABCD = \(AB\times BC\)
  10. ⇒ work done in the process of ABCD = \((3V_o-V_o)\times (2 P_o-P_o)\)
  11. ⇒ work done in the process of ABCD = \(2V_o\times P_o\)
  12. ⇒ work done in the process of ABCD = \(2V_o P_o\)
  13. Here we can see that the process is in an anti-clockwise direction, therefore;
  14. work done in the process of ABCD = \(-2V_o P_o\)
  15. Hence, option 2) is the correct answer.

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students 1 g of water, of volume 1 cm 3 at 100°C, is converted into steam at same temperature under normal atmospheric pressure (≃1 × 10 5 Pa).

  • CONCEPT:
  • According to the first law of thermodynamics we have;
  • Q = ΔU + W
  • Here we have Q is heated, ΔU is the change in internal energy and W is the work done.
  • CALCULATION:
  • Given: mass, m = 1 g
  • Latent heat of vaporization, L = 2256 J/g
  • Pressure, P = 1 × 10 5 Pa
  • The volume, \((V_2-V_1)\) = 1671 cm 3
  • As we know that
  • Q = ΔU + W -(1)
  • The work done, W = PdV
  • and heat Q = mL
  • Now, on putting the values in equation (1) we have;
  • mL = ΔU + P(V2 – V1) -(2)
  • Now, on putting all the given values in (2) we have;
  • \(1 \times 2256 = Δ U +1 \times 10^5 (1671 \times 10^ )\)
  • ⇒ ΔU = 2089 J
  • Hence, option 4) is the correct answer.

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students A system absorbs 50 J of heat and does 11 J of work in a process. The system follows a different thermodynamic path between the same initial and final states and does 15 J work, the heat transferred in the process is

  1. Concept :
  2. The first law of thermodynamics:
  3. It states that heat is a basic form of energy and all the thermodynamic processes are based on the conservation of energy.
  4. ⇒ Q = ΔU + W
  5. where Q is heat energy, ΔU is internal energy change and W is work done.
  6. ​ Calculation :
  7. Given:
  8. Heat absorbed by system Q = 50 J, Work Done by the system W 1 = 11 J,
  9. ⇒ Q = ΔU + W
  10. ∴ ΔU = Q – W
  11. ∴ ΔU = 50 – 11 = 39 J

As another statement says that system follows a different thermodynamic path between the same initial and final states and does 15 J work here as work done by the system.

​⇒ Supplied heat to the system is a change in internal energy plus work done to the system. ∴ Supplied heat = 39 + 15 = 54 J India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students _ of thermodynamics is used to understand the concept of energy conservation.

  1. Zeroth law
  2. First law
  3. Second law
  4. None of the above

Concept:

The zeroth law of thermodynamics states that if two thermodynamic systems are each in thermal equilibrium with a third, then they are in thermal equilibrium with each other.

This law is the basis for the temperature measurement,

The first law of thermodynamics states that energy cannot be created or destroyed in an isolated system; energy can only be transferred or changed from one form to another.

The first law of thermodynamics is a restatement of the law of conservation of energy i.e., According to the first law of Thermodynamics: ΔQ = ΔW + ΔU

Now the First Law of Thermodynamics helped us in understanding the principle of conservation of energy, whereas according to the Second Law of thermodynamics for natural system heat always flows in one direction (higher temperature to lower temperature body) unless it aided by an external factor.

  • And to measure the direction of force we use term entropy which can be expressed as
  • \( }S = \;\smallint \frac } \)
  • ΔQ = heat exchange
  • ΔW = work done due to expansion
  • ΔU = internal energy of the system
  • ΔS = change in entropy
  • T = temperature
  • Explanation:
  • As explained above according to the first law of thermodynamics energy cannot be created or destroyed in an isolated system, energy can only be transferred or changed from one form to another.
  • This is the ideal statement which is used in thermodynamics for explaining the concept of energy conservation among systems and surrounding.
  • Hence option 2 is correct among all
  • Tricks to remember:
  • This is the conclusive point for all three laws of thermodynamics.
  • Zeroth law – Concept of temperature
  • First law – Concept of internal energy/ energy conservation
  • Second law – Concept of entropy/ heat flow

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students The heat given to an ideal gas in isothermal conditions is used to:

  1. increase temperature
  2. do external work
  3. increase temperature and in doing external work
  4. increase internal energy

Option 2 : do external work CONCEPT : First Law of Thermodynamics:

  • It is a statement of conservation of energy in the thermodynamical process,
  • According to it heat given to a system (ΔQ) is equal to the sum of the increase in its internal energy (ΔU) and the work done (ΔW) by the system against the surroundings.

i.e ΔQ = ΔU + ΔW

It makes no distinction between work and heat as according to it the internal energy (and hence temperature) of a system may be increased either by adding heat to it or doing work on it or both,

EXPLANATION :

  • When a thermodynamic system undergoes a physical change in such a way that its temperature remains constant, then the change is known as an isothermal process,
  • As we know that, the internal energy of the system is a function of temperature alone, so in the isothermal process, the change in internal energy is zero.

⇒ ΔQ = 0 + ΔW = ΔW

Therefore, the heat given to an ideal gas in isothermal conditions is used to do external work, Hence option 2 is correct.

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students 110 joule of heat is added to a gaseous system, whose internal energy is 40 J. Then the amount of external work done is Concept :

  • The first law of thermodynamics is a restatement of the law of conservation of energy. It states that energy cannot be created or destroyed in an isolated system; energy can only be transferred or changed from one form to another.
  • When heat energy is supplied to a thermodynamic system or any machine.
  • Two things may occur:
    • The internal energy of the System or machine may change.
    • The system may do some external work,
  1. According to the first law of Thermodynamics :
  2. ΔQ = ΔW + ΔU
  3. Where ΔQ = Heat supplied to the system or heat exchange, ΔW = work done by the system, ΔU = change in internal energy of the system
  4. Explanation :
  5. Given that, ΔQ = 110 J, ΔU = 40 J
  6. According to the first law of thermodynamics :
  7. ΔQ = ΔW + ΔU
  8. ΔU = ΔQ – ΔW
  9. 40 J = 110 J – ΔW
  10. ΔW = 110 – 40 = 70 J
  11. Then the amount of external work done is 70 J.

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students If we had a system on which 10 J of work is done and the internal energy change of the system is 3.5 J, in this case, the amount of heat loss/gain by the system will be?

  1. +6.5 J
  2. -6.5 J
  3. ​+2.85 J
  4. +13.5 J

CONCEPT :

The first law of thermodynamics is a restatement of the law of conservation of energy. It states that energy cannot be created or destroyed in an isolated system; energy can only be transferred or changed from one form to another.

When heat energy is supplied to a gas, two things may occur:

  • The internal energy of the gas may change
  • The gas may do some external work by expanding

According to the first law of Thermodynamics : ΔQ = ΔW + ΔU i.e., When a process is executed by a system, the change in stored energy of the system is numerically equal to the net heat interaction minus the network interaction during the process:

  • Here, ΔQ = heat exchange, ΔW = work done due to expansion, ΔU = internal energy of the system
  • CALCULATION :
  • Given that,
  • Work done on the system, ΔW = -10J
  • The internal energy change of the system, ΔU = 3.5 J

Thus from the above explanation, we can see that according to the first law of thermodynamics heat exchange for a system is the sum of work done by the system and internal energy of molecule or atoms.

i.e., ΔQ = ΔW + ΔU ΔQ = -10 + 3.5 = -6.5 J

  • Here positive sign denotes that heat energy is entering the system, whereas a negative sign denotes that heat energy is leaving the system
  • Similarly, if work is done by the system then it is denoted by a positive sign and a negative sign denotes when work is done on the system,
  1. thus option 2 is correct among all.
  2. Confusion Points
  3. In chemistry sign convention used for work done by or on system are opposite compared to physics

i.e., If work is done on the system, its sign is positive, If work is done by the system, its sign is negative India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students During an adiabatic expansion of 3 moles of a gas, the change in internal energy was found to be equal to – 100 J.

  • An adiabatic process is where no heat is exchanged between the system and surrounding,
  • The first law of thermodynamics: It states that energy can neither be created nor destroyed; energy can only be transferred or changed from one form to another.
    • ​For a system at thermodynamic equilibrium, the change in internal energy is equal to the difference in heat transfer of the system and work done on it. This is given by
  • ​ΔU = Q – W
  • Where ​ΔU is the change in internal energy, Q is the heat exchanged in the system and W is the work done during the thermodynamic process.
  • EXPLANATION :
  • Given that:
  • Change in internal energy, ΔU = -100 J
  • Since it is an adiabatic process, the heat exchanged will be zero, ⇒ Q = 0
  • ​ΔU = Q – W
  • -100 = 0 – W
  • Work done, W = 100 J

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students A particular system gains 200 kJ of heat, and results in a change in internal energy of 129 kJ. Calculate the work done.

  1. + 329 kJ
  2. + 71 kJ
  3. – 329 kJ
  4. – 71 kJ

The correct answer is option 2) i.e. + 71 kJ CONCEPT :

  • The first law of thermodynamics: It states that energy can neither be created nor destroyed, but can only be converted from one form to another.
    • The heat energy supplied to a thermodynamic system increases its internal energy and the remaining heat energy is converted into the work done by the system.
    • If dQ is the heat given to the thermodynamic system and dU is its change in internal energy and dW is the work done by the system, then first of law of thermodynamics gives
  1. dQ = dW + dU
  2. CALCULATION :
  3. Given that:
  4. Heat supplied, dQ = 200 kJ
  5. Change in internal energy, dU = 129 kJ
  6. From first law of thermodynamics, dQ = dW + dU
  7. 200 = dW + 129 ⇒ dW = 200 – 129 = 71 kJ

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students The internal energy change for a system is + 20 Cal and the work done is – 200 Cal. Find the heat exchanged between the system and the surrounding.

  1. 220 Cal
  2. – 220 Cal
  3. – 180 Cal
  4. + 180 Cal

CONCEPT :

  • The first law of thermodynamics is a restatement of the law of conservation of energy. It states that energy cannot be created or destroyed in an isolated system; energy can only be transferred or changed from one form to another.
  • When heat energy is supplied to a thermodynamic system or any machine: Two things may occur:
    • The internal energy of the System or machine may change.
    • The system may do some external work,
  • According to the first law of Thermodynamics :
  • ΔQ = ΔW + ΔU
  • Where ΔQ = Heat supplied to the system, ΔW = work done by the system, and ΔU = change in internal energy of the system
  • EXPLANATION :
  • Given that:
  • ΔW = – 200 Cal and ΔU = + 20 Cal
  • According to the first law of Thermodynamics :
  • Heat exchanged (ΔQ) = ΔW + ΔU = – 200 + 20 = – 180 Cal

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students The first law of thermodynamics in an isothermal process is represented by- (ΔQ = heat exchanged, Δ W = work done, and ΔU = Internal energy change).

  1. ΔQ = ΔU
  2. ΔW = ΔU
  3. ΔQ = ΔU – ΔW
  4. ΔQ = ΔW

CONCEPT :

  • The first law of thermodynamics is a restatement of the law of conservation of energy. It states that energy cannot be created or destroyed in an isolated system; energy can only be transferred or changed from one form to another.
  • When heat energy is supplied to a thermodynamic system or any machine: Two things may occur:
    • The internal energy of the System or machine may change.
    • The system may do some external work,
  1. According to the first law of Thermodynamics :
  2. ΔQ = ΔW + ΔU
  3. Where ΔQ = Heat supplied to the system, ΔW = work done by the system, ΔU = change in internal energy of the system

Isothermal process : When a thermodynamic system undergoes a physical change in such a way that its temperature remains constant, then the change is known as an isothermal process,

  • Change in temperature = ΔT = 0
  • The change in internal energy ( ΔU ) is given by:
  • ΔU = n C v ΔT
  • Where C v = molar specific heat capacity at the constant volume, n is the number of moles
  • EXPLANATION :
  • In an isothermal process,
  • ΔT = 0
  • ΔU = n C v ΔT = 0
  • According to the first law of Thermodynamics :
  • ΔQ = ΔW + ΔU
  • ΔQ = ΔW + 0
  • Hence ΔQ = ΔW
  • So option 4 is correct.

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students The heat given to a thermodynamic system is 200 J and work done by the system is 100 J. Find the change in internal energy of the system. CONCEPT :

  • T he first law of thermodynamics gives the relationship betw een heat, work, and internal energy.
  • The first law of thermodynamics applies the conservation of energy principle to systems.
  • The first law of thermodynamics states that the change in internal energy of a closed system equals the net heat transfer into the system minus the net work done by the system.
  1. In equation form, the first law of thermodynamics is given by:
  2. Q = ΔU + W
  3. where Q is the sum of all heat transfers into and out of the system, W is the net work done by the system and ΔU is the change in internal energy,
  4. CALCULATION :
  5. Given that:
  6. Heat supplied to the system Q = +200 J
  7. Work done by the system W = +100 J
  8. By the first law of thermodynamics Q = ΔU + W
  9. 200 = ΔU + 100
  10. ΔU = 100 J
  11. So the correct answer is option 3.
  12. Important Points
  13. Sign convention:
  • ΔQ = Positive (Heat supplies to the system)
  • ΔQ = Negative (Heat rejected from the system)
  • ΔW = Positive (Work done by the system)
  • ΔW = Negative (Work done on the system).

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students A diatomic gas does 80 J of work when compressed isobarically. The heat given to the gas during this process is CONCEPT:

Work: The energy required to move a system or body or anything against a force is called work.

  • Isobaric Process (Constant Pressure): Work done in an isobaric process is given by:
  • ΔW = P ΔV
  • where W is Work done, P is the pressure and ΔV is change in volume.
  • The ideal gas equation is given by:
  • P V = n R T
  • Where P is pressure, V is volume, n is the number of moles, R is gas constant and T is temperature.
  • According to the first law of Thermodynamics :
  • ΔQ = ΔW + ΔU
  • Where ΔQ = Heat supplied to the system, ΔW = work done by the system, and ΔU = change in internal energy of the system
  • The change in internal energy ( ΔU ) is given by:
  • ΔU = n C v ΔT
  • Where C v = fR/2 = molar-specific heat capacity at the constant volume, f is the degree of freedom.
  • CALCULATION :
  • For diatomic molecule,
  • γ = 7/5, and Cv = R/(γ -1) = 5R/2
  • ∴ ΔU = n C v ΔT = n (5R/2) ΔT = 5 nRΔT/2
  • Given that:
  • For isobaric process :
  • Work done (Δ W) = 80 J = P ΔV
  • Since P V = n R T
  • So P ΔV = n R ΔT
  • ΔU = 5 nRΔT/2 = 5 (P ΔV)/2 = 5 × 80/2 = 200 J
  • Applying first law of thermodynamics:
  • ΔQ = ΔW + ΔU = 80 + 200 = 280 J
  • Heat given to the gas = 280 J
  • So option 3 is correct.
  • Additional Information
  • A diatomic gas does 80 J of work when compressed isobarically. The heat is given to the gas during this process,
  • Q = n C p ΔT
  • Q = n γ C v ΔT
  • Q = n γ C v ΔT =
  • Q = γ n (5R/2) ΔT = 5 nRγΔT/2
  • Q = 2.5 nR γΔT
  • For diatomic gas,
  • γ = (f + 2)/f = (5 + 2)/5 = 7/5
  • Since P V = n R T
  • So P ΔV = n R ΔT
  • ⇒ Q = 7/5 × 2.5 P ΔV
  • ⇒ Q = 3.5 × 80 = 280 J

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.5 Crore+ Students : First law of thermodynamics MCQ – Objective Question Answer for First law of thermodynamics Quiz – Download Now!

Is Say’s law consistent with quantity theory of money?

Assumptions: – The classical quantity theory of money is based on two fundamen­tal assumptions: First is the operation of Say’s Law of Market. Say’s law states that, “Supply creates its own demand.” This means that the sum of values of all goods produced is equivalent to the sum of values of all goods bought.

Which system is always consistent Mcq?

Homogeneous system of linear equations is always consistent.

Which of the following is the best example of the law of supply?

Answer and Explanation: A sandwich shop increases the number of sandwiches they supply every day when the price is increased. Law of supply states that as the price of good increases the quantity supplied by the producer also increases.

Which statements are true according to the law of supply quizlet?

Which statements are true according to the law of supply? A decrease in price leads to a decrease in supply. An increase in price leads to an increase in supply. Which phrase describes the substitution effect?

Which relationship is the best example of the law of supply quizlet?

Which relationship is the BEST example of the Law of Supply? The quantity of a good supplied rises as the price rises.

Which statement is consistent with the law of demand select?

Which statement is consistent with the law of demand? A reduction in market price will lead to an increase in quantity demanded.

Which of the following is consistent with the law of demand a A decrease in the price of a gallon of milk causes a decrease in the quantity of milk demanded?

The correct Option is (iii) An increase in the price of soda causes a decrease in the quantity of soda demanded. The law of demand expresses the inverse functional relationship between the variables such as price and quantity demanded of a commodity.

Which is the correct law of demand?

The law of demand states that as the price of a good decreases, the quantity demanded of that good increases. In other words, the law of demand states that the demand curve, as a function of price and quantity, is always downward sloping.