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Ideal Gas Equation

Which of the ...

Question

Which of the following relationships for various gas laws is not correct?

A

V_{t} = V_{0} + \frac{V_{0}}{273} \times t

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B

\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{1}} (c o n s t a n t P)

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C

\frac{P_{1}}{T_{1}} = \frac{P_{2}}{T_{1}} (c o n s t a n t V)

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D

\frac{P_{1} T_{1}}{V_{1}} = \frac{P_{2} T_{2}}{V_{2}}

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Solution

The correct option is A $\frac{P_{1} T_{1}}{V_{1}} = \frac{P_{2} T_{2}}{V_{2}}$
According to ideal gas equation $P V = n R T$
$∴ P_{1} V_{1} = n R T_{1}$ or $P_{1} V_{1} / T_{1} = n R$
$P_{2} V_{2} = n R T_{2}$ or $P_{2} V_{2} / T_{2} = n R$
$\Rightarrow \frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$
Hence $\frac{P_{1} T_{1}}{V_{1}} = \frac{P_{2} T_{2}}{V_{2}}$ is incorrect

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Similar questions

Q. Which gas law is summarized with the following equation?

(P_{1} V_{1}) / T_{1} = (P_{2} V_{2}) / T_{2}

For an ideal gas, an illustration of three different paths

A

(B + C)

(D + E)

from an initial state

P_{1}

V_{1}

T_{1}

to a final state

P_{2}

V_{2}

T_{1}

is shown in the given figure.
Path

A

represents a reversible Isothermal expansion from

P_{1}

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(B + C)

reperesents a reversible adiabatic expansion

(B)

P_{1} V_{1}

T_{1}

P_{3}

V_{2}

T_{2}

followed by reversible heating the gas at constant volume

(C)

P_{3}

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T_{2}

P_{2}

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T_{1}

(D + E)

represents a reversible expansion at constant pressure

P_{1} (D)

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T_{1}

P_{1}

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T_{3}

followed by a reversible cooling at constant volume

V_{2} (E)

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P_{2}

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Δ S

(D + E) ?

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v_{1}, v_{2} a n d v_{3}

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