The heat required to raise the temperature of $1 \ mol$ of a substance by $1^{\circ}C$ is called:

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 $kJ \ mol^{-1}$?

$A$ piece of metal weighing $100 \, g$ is heated to $80^{\circ} C$ and dropped into $1 \, kg$ of cold water in an insulated container at $15^{\circ} C$. If the final temperature of the water in the container is $15.69^{\circ} C$,the specific heat of the metal in $J / g \cdot ^{\circ} C$ is

The heat required to raise the temperature of a body by $1 \, K$ is called

Heat capacity $(C_{p})$ is an extensive property but specific heat $(c)$ is an intensive property. What will be the relation between $C_{p}$ and $c$ for $1 \ mol$ of water?

$4.48 \ L$ of an ideal gas at $1 \ atm$ and $273 \ K$ requires $12 \ cal$ to raise the temperature by $15 \ ^\circ C$ at constant volume. The $C_p$ of the gas is $... \ cal \ mol^{-1} K^{-1}$.