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Molar heat capacity $\left(C_p\right)$ of water at constant pressure is $75 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$. The increase in temperature (in K) of $100 \mathrm{~g}$ of water when $1 \mathrm{~kJ}$ of heat is supplied to it is
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$2.4$
Molar heat capacity is the amount of heat required to raise the temperature of 1 mole of a substance by $1^{\circ} \mathrm{C}$.
$\begin{aligned} \therefore \quad \Delta H & =n C_p \Delta T \\ 1000 & =\frac{100}{18} \times 75 \times \Delta T \\ \Delta T & =\frac{180}{75}=2.4^{\circ}\end{aligned}$
$\begin{aligned} \therefore \quad \Delta H & =n C_p \Delta T \\ 1000 & =\frac{100}{18} \times 75 \times \Delta T \\ \Delta T & =\frac{180}{75}=2.4^{\circ}\end{aligned}$
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