The P-T graph as given below was observe for a process on an ideal gas, which of the following statement is true?

w = +ve,

Δ H

= +ve

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w = -ve,

Δ H

= -ve

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w = -ve,

Δ H

= +ve

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w = +ve,

Δ H

= -ve

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Solution

The correct option is D w = -ve, $Δ H$ = +ve
$Δ H$ = $n C_{p} Δ T$

If temperature changes are positive then enthalpy change will be positive.

In this graph temperature changes is positive then enthalpy change is positive.

We know, $V \propto T$

If the temperature is increased then the volume of gas will be increased.

$W = - P (V_{2} - V_{1})$

As volume increases so $(V_{2} - V_{1})$ is positive

so work done is negative.

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