148114 The internal energy change in a system that has a absorbed 2 kcal of heat and done $500 \mathrm{~J}$ of work is

148115 Two moles of a monoatomic ideal gas is confined in a container and is heated such that its temperature increases by $10^{\circ} \mathrm{C}$. The approximate change in its internal energy is $(\mathrm{R}=8.31 \mathrm{~J} / \mathrm{mole}-\mathrm{K})$

148117 The latent heat of vaporization of water is 2240 $\mathrm{J} / \mathrm{g}$. If the work done in the process of vaporization of $1 \mathrm{~g}$ is $168 \mathrm{~J}$, then increase in internal energy is

148118 A system is given 300 calories of heat and it does 600 joules of work. How much does the internal energy of the system change in this process? $(\mathrm{J}=\mathbf{4 . 1 8} \mathrm{Joules} / \mathrm{cal})$

148114 The internal energy change in a system that has a absorbed 2 kcal of heat and done $500 \mathrm{~J}$ of work is

148115 Two moles of a monoatomic ideal gas is confined in a container and is heated such that its temperature increases by $10^{\circ} \mathrm{C}$. The approximate change in its internal energy is $(\mathrm{R}=8.31 \mathrm{~J} / \mathrm{mole}-\mathrm{K})$

148117 The latent heat of vaporization of water is 2240 $\mathrm{J} / \mathrm{g}$. If the work done in the process of vaporization of $1 \mathrm{~g}$ is $168 \mathrm{~J}$, then increase in internal energy is

148118 A system is given 300 calories of heat and it does 600 joules of work. How much does the internal energy of the system change in this process? $(\mathrm{J}=\mathbf{4 . 1 8} \mathrm{Joules} / \mathrm{cal})$

148114 The internal energy change in a system that has a absorbed 2 kcal of heat and done $500 \mathrm{~J}$ of work is

148115 Two moles of a monoatomic ideal gas is confined in a container and is heated such that its temperature increases by $10^{\circ} \mathrm{C}$. The approximate change in its internal energy is $(\mathrm{R}=8.31 \mathrm{~J} / \mathrm{mole}-\mathrm{K})$

148117 The latent heat of vaporization of water is 2240 $\mathrm{J} / \mathrm{g}$. If the work done in the process of vaporization of $1 \mathrm{~g}$ is $168 \mathrm{~J}$, then increase in internal energy is

148118 A system is given 300 calories of heat and it does 600 joules of work. How much does the internal energy of the system change in this process? $(\mathrm{J}=\mathbf{4 . 1 8} \mathrm{Joules} / \mathrm{cal})$

148114 The internal energy change in a system that has a absorbed 2 kcal of heat and done $500 \mathrm{~J}$ of work is

148115 Two moles of a monoatomic ideal gas is confined in a container and is heated such that its temperature increases by $10^{\circ} \mathrm{C}$. The approximate change in its internal energy is $(\mathrm{R}=8.31 \mathrm{~J} / \mathrm{mole}-\mathrm{K})$

148117 The latent heat of vaporization of water is 2240 $\mathrm{J} / \mathrm{g}$. If the work done in the process of vaporization of $1 \mathrm{~g}$ is $168 \mathrm{~J}$, then increase in internal energy is

148118 A system is given 300 calories of heat and it does 600 joules of work. How much does the internal energy of the system change in this process? $(\mathrm{J}=\mathbf{4 . 1 8} \mathrm{Joules} / \mathrm{cal})$