The specific heat of hydrogen gas at constant | vedclass

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(B) According to the First Law of Thermodynamics,$\Delta Q = \Delta U + \Delta W$.For a process at constant pressure,the work done by the gas is $\Del

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$10^4 	ext{ cal}$

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(B) According to the First Law of Thermodynamics,$\Delta Q = \Delta U + \Delta W$.For a process at constant pressure,the work done by the gas is $\Delta W = \Delta Q_P - \Delta U$.Since the change in internal energy $\Delta U$ is equal to the heat supplied at constant volume,$\Delta U = \Delta Q_V = m C_V \Delta T$.The heat supplied at constant pressure is $\Delta Q_P = m C_P \Delta T$.Therefore,the work done is $\Delta W = m(C_P - C_V) \Delta T$.Given: $m = 1 	ext{ kg}$,$C_P = 3.4 	imes 10^3 	ext{ cal/kg } ^oC$,$C_V = 2.4 	imes 10^3 	ext{ cal/kg } ^oC$,and $\Delta T = 20^oC - 10^oC = 10^oC$.Substituting the values: $\Delta W = 1 	imes (3.4 	imes 10^3 - 2.4 	imes 10^3) 	imes 10$.$\Delta W = 1 	imes (1.0 	imes 10^3) 	imes 10 = 10^4 	ext{ cal}$.

The specific heat of hydrogen gas at constant pressure is $C_P = 3.4 \times 10^3 \text{ cal/kg } ^oC$ and at constant volume is $C_V = 2.4 \times 10^3 \text{ cal/kg } ^oC$. If $1 \text{ kg}$ of hydrogen gas is heated from $10^oC$ to $20^oC$ at constant pressure,the external work done by the gas is:

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