Molar heat capacity of water in equilibrium with ice at constant pressure is

The energy required to increase the temperature of $180 \ g$ of liquid water from $10^{\circ} C$ to $15^{\circ} C$ is $3765 \ J$. What is $C_{p}$ of water in $J \ mol^{-1} \ K^{-1}$ ? $(H_2O = 18 \ u)$

Explain Heat Capacity.

For a reaction $H_{2(g)} + \frac{1}{2}O_{2(g)} \longrightarrow H_2O_{(l)}$; $\Delta C_p = 32 \ J \ K^{-1}$,$\Delta H$ at $27 \ ^oC = -285.8 \ kJ \ mol^{-1}$. What will be the value of $\Delta H$ at $127 \ ^oC$ in $kJ \ mol^{-1}$?

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 $...... \ K$.

At constant volume,$4 \; mol$ of an ideal gas when heated from $300 \; K$ to $500 \; K$ changes its internal energy by $5000 \; J$. The molar heat capacity at constant volume is ............... $J \; mol^{-1} \; K^{-1}$