The molar heat capacity of water at constant | vedclass

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(B) The formula for heat supplied at constant pressure is $Q = n 	imes C_p 	imes \Delta T$. Here,$n$ is the number of moles of water,$C_p$ is the mo

Vedclass · Accepted Answer

$2.4$

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(B) The formula for heat supplied at constant pressure is $Q = n 	imes C_p 	imes \Delta T$. Here,$n$ is the number of moles of water,$C_p$ is the molar heat capacity at constant pressure,and $\Delta T$ is the change in temperature. First,calculate the number of moles of water: $n = \frac{	ext{mass}}{	ext{molar mass}} = \frac{100 \, g}{18 \, g \, mol^{-1}} = \frac{100}{18} \, mol$. Given $Q = 1.0 \, kJ = 1000 \, J$ and $C_p = 75 \, J \, K^{-1} \, mol^{-1}$. Substituting the values into the equation: $1000 = (\frac{100}{18}) 	imes 75 	imes \Delta T$. Solving for $\Delta T$: $\Delta T = \frac{1000 	imes 18}{100 	imes 75} = \frac{10 	imes 18}{75} = \frac{180}{75} = 2.4 \, K$.

The molar heat capacity of water at constant pressure is $75 \, J \, K^{-1} \, mol^{-1}$. When $1.0 \, kJ$ of heat is supplied to $100 \, g$ of water,which is free to expand,the increase in temperature of water is $...... \, K$.

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