When 128 , g of oxygen gas is heated from 0 , | vedclass

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(B) The molar mass of oxygen $(O_2)$ is $32 \, g/mol$.Number of moles $(n)$ = $\frac{128 \, g}{32 \, g/mol} = 4 \, mol$.Change in temperature $(\Delta

Vedclass · Accepted Answer

$2000 \, cal, 2800 \, cal$

Vedclass · Answer

(B) The molar mass of oxygen $(O_2)$ is $32 \, g/mol$.Number of moles $(n)$ = $\frac{128 \, g}{32 \, g/mol} = 4 \, mol$.Change in temperature $(\Delta T)$ = $100 \, ^oC - 0 \, ^oC = 100 \, K$.The change in internal energy is given by $\Delta U = n 	imes C_v 	imes \Delta T$.$\Delta U = 4 \, mol 	imes 5 \, cal \, mol^{-1} \, K^{-1} 	imes 100 \, K = 2000 \, cal$.The change in enthalpy is given by $\Delta H = n 	imes C_p 	imes \Delta T$.$\Delta H = 4 \, mol 	imes 7 \, cal \, mol^{-1} \, K^{-1} 	imes 100 \, K = 2800 \, cal$.Thus,the values of $\Delta U$ and $\Delta H$ are $2000 \, cal$ and $2800 \, cal$ respectively.

When $128 \, g$ of oxygen gas is heated from $0 \, ^oC$ to $100 \, ^oC$,the average values of $C_v$ and $C_p$ are $5 \, cal \, mol^{-1} \, K^{-1}$ and $7 \, cal \, mol^{-1} \, K^{-1}$ respectively. Find the values of $\Delta U$ and $\Delta H$.

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