In an experiment on the specific heat of a metal, a $0.20 \;kg$ block of the metal at $150\,^{\circ} C$ is dropped in a copper calorimeter (of water equivalent $0.025 \;kg$ ) containing $150 \;cm ^{3}$ of water at $27\,^{\circ} C$. The final temperature is $40\,^{\circ} C$. Compute the specific heat of the metal. If heat losses to the surroundings are not negligible, is your answer greater or smaller than the actual value for specific heat of the metal?

$\mathrm{C}_{\mathrm{v}}$ and $\mathrm{C}_{\mathrm{p}}$ denote the molar specific heat capacities of a gas at constant volume and constant pressure, respectively. Then

$(A)$ $\mathrm{C}_{\mathrm{p}}-\mathrm{C}_{\mathrm{v}}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas

$(B)$ $\mathrm{C}_{\mathrm{p}}+\mathrm{C}_{\mathrm{v}}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas

$(C)$ $\mathrm{C}_{\mathrm{p}} / \mathrm{C}_{\mathrm{v}}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas

$(D)$ $\mathrm{C}_{\mathrm{p}} \cdot \mathrm{C}_v$ is larger for a diatomic ideal gas than for a monoatomic ideal gas

A bullet of mass $5\, g$, travelling with a speed of $210$ $m / s ,$ strikes a fixed wooden target. One half of its kinetic energy is converted into heat in the bullet while the other half is converted into heat in the wood. The rise of temperature of the bullet if the specific heat of its material is $0.030\, cal /\left( g -{ }^{\circ} C \right)$ $\left(1\, cal =4.2 \times 10^{7}\, ergs \right)$ close to$…….^oC$

In supplying $400$ calories of heat to a system, the work done will be

What is heat capacity of a substance ?