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Standard XIII

Chemistry

First Law of Thermodynamics

3000 J of hea...

Question

$3000 J$ of heat is given to a gas at constant pressure of $2 \times 10^{5} {N/m}^{2}$ If its volume increases by $10$ litres during the process find the change in the internal energy of the gas.

- 1000 J

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1000 J

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- 2000 J

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2000 J

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Solution

The correct option is B $1000 J$
Heat given to the system $△ Q = 3000 J$
pressure applied = $2 \times 10^{5} {N/m}^{2})$
$W = P △ V = (2 \times 10^{5} {N/m}^{2}) (10 \times 10^{- 3} m^{3})$
$= 2 \times 10^{3} J$
from first law of thermodynamic,
$△ U = △ Q - W = 3000 - 2000 = 1000 J$

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First Law of Thermodynamics

Standard XIII Chemistry

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3000 J of heat is given to a gas at constant pressure of 2×105 N/m2 If its volume increases by 10 litres during the process find the change in the internal energy of the gas.

The correct option is B 1000 JHeat given to the system △Q=3000 J pressure applied = 2×105 N/m2) W=P△V=(2×105 N/m2)(10×10−3 m3) =2×103 J from first law of thermodynamic, △U=△Q−W=3000−2000=1000 J

$3000 J$ of heat is given to a gas at constant pressure of $2 \times 10^{5} {N/m}^{2}$ If its volume increases by $10$ litres during the process find the change in the internal energy of the gas.

The correct option is B $1000 J$
Heat given to the system $△ Q = 3000 J$
pressure applied = $2 \times 10^{5} {N/m}^{2})$
$W = P △ V = (2 \times 10^{5} {N/m}^{2}) (10 \times 10^{- 3} m^{3})$
$= 2 \times 10^{3} J$
from first law of thermodynamic,
$△ U = △ Q - W = 3000 - 2000 = 1000 J$