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Standard XII

Chemistry

Heat of Reaction

An ideal gas ...

Question

An ideal gas is expanded irreversible against $10$ bar pressure from $20$ litre to $30$ litre. Calculate ' $q$ ' if process is isoenthalpic.

0

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+ 100 J

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- 100 J

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+ 10 k J

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Solution

The correct option is D $+ 10 k J$
$W_{i r r} = - P_{o p p} (V_{2} - V_{1})$
$= - 10 b a r (30 - 20) l i t$
$= - 9.869 a t m \times 10 l i t$
$= - 98.69 l i t - a t m = - 9999.76 \approx - 10 k J$
Since, $Δ H = 0, q = - W_{i r r}$
$q = 10 k J$

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An ideal gas is expanded irreversible against 10 bar pressure from 20 litre to 30 litre. Calculate 'q' if process is isoenthalpic.

The correct option is D +10kJWirr=−Popp(V2−V1) =−10bar(30−20)lit =−9.869atm×10lit =−98.69lit−atm=−9999.76≈−10kJSince, ΔH=0,q=−Wirr q=10kJ

An ideal gas is expanded irreversible against $10$ bar pressure from $20$ litre to $30$ litre. Calculate ' $q$ ' if process is isoenthalpic.

The correct option is D $+ 10 k J$
$W_{i r r} = - P_{o p p} (V_{2} - V_{1})$
$= - 10 b a r (30 - 20) l i t$
$= - 9.869 a t m \times 10 l i t$
$= - 98.69 l i t - a t m = - 9999.76 \approx - 10 k J$
Since, $Δ H = 0, q = - W_{i r r}$
$q = 10 k J$