146422 If a thermometer reads melting point of water as $20^{\circ} \mathrm{C}$ and boiling point as $180^{\circ} \mathrm{C}$, how much does the thermometer read when the actual temperature is $60^{\circ} \mathrm{C}$ ?

146423 A rigid insulated box is divided into two parts with a partition. One part is occupied by 1 gram mole of an ideal gas at temperature $T_{1}$ and the other by 2 gram moles of the same ideal gas at temperature $T_{2}$. When the partition is removed, what is the final equilibrium temperature $T$ of the mixture?

146425 The temperature of a gas contained in a closed vessel of constant volume increases by $1^{0} \mathrm{C}$ when the pressure of the gas is increased by $1 \%$. The initial temperature of the gas is:

146426 $0.1 \mathrm{~m}^{3}$ of water at $80^{\circ} \mathrm{C}$ is mixed with $0.3 \mathrm{~m}^{3}$ of water at $60^{\circ} \mathrm{C}$. The final temperature of the mixture is :

146422 If a thermometer reads melting point of water as $20^{\circ} \mathrm{C}$ and boiling point as $180^{\circ} \mathrm{C}$, how much does the thermometer read when the actual temperature is $60^{\circ} \mathrm{C}$ ?

146423 A rigid insulated box is divided into two parts with a partition. One part is occupied by 1 gram mole of an ideal gas at temperature $T_{1}$ and the other by 2 gram moles of the same ideal gas at temperature $T_{2}$. When the partition is removed, what is the final equilibrium temperature $T$ of the mixture?

146425 The temperature of a gas contained in a closed vessel of constant volume increases by $1^{0} \mathrm{C}$ when the pressure of the gas is increased by $1 \%$. The initial temperature of the gas is:

146426 $0.1 \mathrm{~m}^{3}$ of water at $80^{\circ} \mathrm{C}$ is mixed with $0.3 \mathrm{~m}^{3}$ of water at $60^{\circ} \mathrm{C}$. The final temperature of the mixture is :

146422 If a thermometer reads melting point of water as $20^{\circ} \mathrm{C}$ and boiling point as $180^{\circ} \mathrm{C}$, how much does the thermometer read when the actual temperature is $60^{\circ} \mathrm{C}$ ?

146423 A rigid insulated box is divided into two parts with a partition. One part is occupied by 1 gram mole of an ideal gas at temperature $T_{1}$ and the other by 2 gram moles of the same ideal gas at temperature $T_{2}$. When the partition is removed, what is the final equilibrium temperature $T$ of the mixture?

146425 The temperature of a gas contained in a closed vessel of constant volume increases by $1^{0} \mathrm{C}$ when the pressure of the gas is increased by $1 \%$. The initial temperature of the gas is:

146426 $0.1 \mathrm{~m}^{3}$ of water at $80^{\circ} \mathrm{C}$ is mixed with $0.3 \mathrm{~m}^{3}$ of water at $60^{\circ} \mathrm{C}$. The final temperature of the mixture is :

146422 If a thermometer reads melting point of water as $20^{\circ} \mathrm{C}$ and boiling point as $180^{\circ} \mathrm{C}$, how much does the thermometer read when the actual temperature is $60^{\circ} \mathrm{C}$ ?

146423 A rigid insulated box is divided into two parts with a partition. One part is occupied by 1 gram mole of an ideal gas at temperature $T_{1}$ and the other by 2 gram moles of the same ideal gas at temperature $T_{2}$. When the partition is removed, what is the final equilibrium temperature $T$ of the mixture?

146425 The temperature of a gas contained in a closed vessel of constant volume increases by $1^{0} \mathrm{C}$ when the pressure of the gas is increased by $1 \%$. The initial temperature of the gas is:

146426 $0.1 \mathrm{~m}^{3}$ of water at $80^{\circ} \mathrm{C}$ is mixed with $0.3 \mathrm{~m}^{3}$ of water at $60^{\circ} \mathrm{C}$. The final temperature of the mixture is :