277367 The weight in gram, of the non-volatile solute urea $\left(\mathrm{NH}_{2} \mathrm{CONH}_{2}\right)$ to be dissolved in $100 \mathrm{~g}$ of water in order to decrease its vapour pressure by $1.8 \%$ is

277368 At a particular temperature, the vapour pressures of two liquids $A$ and $B$ are respectively 120 and $180 \mathrm{~mm}$ of mercury. If 2 moles of $A$ and 3 moles of $B$ are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm of mercury)

277369 What will be the freezing point of a $1 \%$ solution of glucose in water, given that molal depression constant for water is $1.84 \mathrm{~K} \mathrm{~kg}$ $\mathrm{mol}^{-1}$ ?

277371 $0.4 \mathrm{~g}$ of $\mathrm{H}_{2}, 22 \mathrm{~g}$ of $\mathrm{CO}_{2}$ and $6.4 \mathrm{~g}$ of $\mathrm{SO}_{2}$ are taken in a container. Total pressure is found to be $1.6 \mathrm{~atm}$. What is the partial pressure of $\mathrm{CO}_{2}$ gas in the mixture?

277373 $58.4 \mathrm{~g}$ of $\mathrm{NaCl}$ and $180 \mathrm{~g}$ of glucose were separately dissolved in $1000 \mathrm{ml}$ of water. Identify the correct statement regarding the elevation of boiling point (b.p) of the resulting solutions.

277367 The weight in gram, of the non-volatile solute urea $\left(\mathrm{NH}_{2} \mathrm{CONH}_{2}\right)$ to be dissolved in $100 \mathrm{~g}$ of water in order to decrease its vapour pressure by $1.8 \%$ is

277368 At a particular temperature, the vapour pressures of two liquids $A$ and $B$ are respectively 120 and $180 \mathrm{~mm}$ of mercury. If 2 moles of $A$ and 3 moles of $B$ are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm of mercury)

277369 What will be the freezing point of a $1 \%$ solution of glucose in water, given that molal depression constant for water is $1.84 \mathrm{~K} \mathrm{~kg}$ $\mathrm{mol}^{-1}$ ?

277371 $0.4 \mathrm{~g}$ of $\mathrm{H}_{2}, 22 \mathrm{~g}$ of $\mathrm{CO}_{2}$ and $6.4 \mathrm{~g}$ of $\mathrm{SO}_{2}$ are taken in a container. Total pressure is found to be $1.6 \mathrm{~atm}$. What is the partial pressure of $\mathrm{CO}_{2}$ gas in the mixture?

277373 $58.4 \mathrm{~g}$ of $\mathrm{NaCl}$ and $180 \mathrm{~g}$ of glucose were separately dissolved in $1000 \mathrm{ml}$ of water. Identify the correct statement regarding the elevation of boiling point (b.p) of the resulting solutions.

277367 The weight in gram, of the non-volatile solute urea $\left(\mathrm{NH}_{2} \mathrm{CONH}_{2}\right)$ to be dissolved in $100 \mathrm{~g}$ of water in order to decrease its vapour pressure by $1.8 \%$ is

277368 At a particular temperature, the vapour pressures of two liquids $A$ and $B$ are respectively 120 and $180 \mathrm{~mm}$ of mercury. If 2 moles of $A$ and 3 moles of $B$ are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm of mercury)

277369 What will be the freezing point of a $1 \%$ solution of glucose in water, given that molal depression constant for water is $1.84 \mathrm{~K} \mathrm{~kg}$ $\mathrm{mol}^{-1}$ ?

277371 $0.4 \mathrm{~g}$ of $\mathrm{H}_{2}, 22 \mathrm{~g}$ of $\mathrm{CO}_{2}$ and $6.4 \mathrm{~g}$ of $\mathrm{SO}_{2}$ are taken in a container. Total pressure is found to be $1.6 \mathrm{~atm}$. What is the partial pressure of $\mathrm{CO}_{2}$ gas in the mixture?

277373 $58.4 \mathrm{~g}$ of $\mathrm{NaCl}$ and $180 \mathrm{~g}$ of glucose were separately dissolved in $1000 \mathrm{ml}$ of water. Identify the correct statement regarding the elevation of boiling point (b.p) of the resulting solutions.

277367 The weight in gram, of the non-volatile solute urea $\left(\mathrm{NH}_{2} \mathrm{CONH}_{2}\right)$ to be dissolved in $100 \mathrm{~g}$ of water in order to decrease its vapour pressure by $1.8 \%$ is

277368 At a particular temperature, the vapour pressures of two liquids $A$ and $B$ are respectively 120 and $180 \mathrm{~mm}$ of mercury. If 2 moles of $A$ and 3 moles of $B$ are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm of mercury)

277369 What will be the freezing point of a $1 \%$ solution of glucose in water, given that molal depression constant for water is $1.84 \mathrm{~K} \mathrm{~kg}$ $\mathrm{mol}^{-1}$ ?

277371 $0.4 \mathrm{~g}$ of $\mathrm{H}_{2}, 22 \mathrm{~g}$ of $\mathrm{CO}_{2}$ and $6.4 \mathrm{~g}$ of $\mathrm{SO}_{2}$ are taken in a container. Total pressure is found to be $1.6 \mathrm{~atm}$. What is the partial pressure of $\mathrm{CO}_{2}$ gas in the mixture?

277373 $58.4 \mathrm{~g}$ of $\mathrm{NaCl}$ and $180 \mathrm{~g}$ of glucose were separately dissolved in $1000 \mathrm{ml}$ of water. Identify the correct statement regarding the elevation of boiling point (b.p) of the resulting solutions.

277367 The weight in gram, of the non-volatile solute urea $\left(\mathrm{NH}_{2} \mathrm{CONH}_{2}\right)$ to be dissolved in $100 \mathrm{~g}$ of water in order to decrease its vapour pressure by $1.8 \%$ is

277368 At a particular temperature, the vapour pressures of two liquids $A$ and $B$ are respectively 120 and $180 \mathrm{~mm}$ of mercury. If 2 moles of $A$ and 3 moles of $B$ are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm of mercury)

277369 What will be the freezing point of a $1 \%$ solution of glucose in water, given that molal depression constant for water is $1.84 \mathrm{~K} \mathrm{~kg}$ $\mathrm{mol}^{-1}$ ?

277371 $0.4 \mathrm{~g}$ of $\mathrm{H}_{2}, 22 \mathrm{~g}$ of $\mathrm{CO}_{2}$ and $6.4 \mathrm{~g}$ of $\mathrm{SO}_{2}$ are taken in a container. Total pressure is found to be $1.6 \mathrm{~atm}$. What is the partial pressure of $\mathrm{CO}_{2}$ gas in the mixture?

277373 $58.4 \mathrm{~g}$ of $\mathrm{NaCl}$ and $180 \mathrm{~g}$ of glucose were separately dissolved in $1000 \mathrm{ml}$ of water. Identify the correct statement regarding the elevation of boiling point (b.p) of the resulting solutions.