277439
Which one is not correct mathematical equation for Dalton's law of partial pressure? Here $p=$ total pressure of gaseous mixture.
1 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}_{\mathrm{i}}^{\mathrm{o}}$, where $\mathrm{x}_{\mathrm{i}}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture $p_{i}^{o}=$ pressure of $i^{\text {th }}$ gas in pure state
4 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}$, where $\mathrm{pi}=$ partial pressure of $\mathrm{i}^{\text {th }}$ gas $\mathrm{xi}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture
Explanation:
Dalton's law of partial pressures according to this law, the total pressure by a mixture of gases is equal to the sum of the partial pressures of each of the constituent gases. i.e. partial pressure of gas $=$ mole fraction of gas in gaseous mixture $\times$ Total pressure of gaseous mixture. $\begin{aligned} & \mathrm{P}_{1}=\mathrm{X}_{1} \mathrm{P} \\ & \mathrm{P}_{2}=\mathrm{X}_{2} \mathrm{P} \\ & \mathrm{P}_{3}=\mathrm{X}_{3} \mathrm{P} \end{aligned}$ $\therefore$ Total pressure $\mathrm{P}=\mathrm{P}_{1}+\mathrm{P}_{2}+\mathrm{P}_{3}$
NEET-17.06.2022
SOLUTIONS
277443
The osmotic pressure of a $5 \%$ (wt./vol) solution of cane sugar at $150^{\circ} \mathrm{C}$ is
277444
A $3 \mathrm{~mL}$ of solution was made by dissolving 20 mg of protein at $0^{0} \mathrm{C}$. The osmotic pressure of the resulting solution is 3.8 torr. The molecular weight of the protein is approximately (in g/mol)
277445
$\mathrm{pH}$ of a $0.1 \mathrm{M}$ monobasic acid is 2. Its osmotic pressure at a given temperature $T(K)$ is (Given that the effective concentration for osmotic pressure is $(1+\alpha) \cdot x$ concentration of acid: $\alpha$ is the dissociation factor)
277439
Which one is not correct mathematical equation for Dalton's law of partial pressure? Here $p=$ total pressure of gaseous mixture.
1 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}_{\mathrm{i}}^{\mathrm{o}}$, where $\mathrm{x}_{\mathrm{i}}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture $p_{i}^{o}=$ pressure of $i^{\text {th }}$ gas in pure state
4 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}$, where $\mathrm{pi}=$ partial pressure of $\mathrm{i}^{\text {th }}$ gas $\mathrm{xi}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture
Explanation:
Dalton's law of partial pressures according to this law, the total pressure by a mixture of gases is equal to the sum of the partial pressures of each of the constituent gases. i.e. partial pressure of gas $=$ mole fraction of gas in gaseous mixture $\times$ Total pressure of gaseous mixture. $\begin{aligned} & \mathrm{P}_{1}=\mathrm{X}_{1} \mathrm{P} \\ & \mathrm{P}_{2}=\mathrm{X}_{2} \mathrm{P} \\ & \mathrm{P}_{3}=\mathrm{X}_{3} \mathrm{P} \end{aligned}$ $\therefore$ Total pressure $\mathrm{P}=\mathrm{P}_{1}+\mathrm{P}_{2}+\mathrm{P}_{3}$
NEET-17.06.2022
SOLUTIONS
277443
The osmotic pressure of a $5 \%$ (wt./vol) solution of cane sugar at $150^{\circ} \mathrm{C}$ is
277444
A $3 \mathrm{~mL}$ of solution was made by dissolving 20 mg of protein at $0^{0} \mathrm{C}$. The osmotic pressure of the resulting solution is 3.8 torr. The molecular weight of the protein is approximately (in g/mol)
277445
$\mathrm{pH}$ of a $0.1 \mathrm{M}$ monobasic acid is 2. Its osmotic pressure at a given temperature $T(K)$ is (Given that the effective concentration for osmotic pressure is $(1+\alpha) \cdot x$ concentration of acid: $\alpha$ is the dissociation factor)
277439
Which one is not correct mathematical equation for Dalton's law of partial pressure? Here $p=$ total pressure of gaseous mixture.
1 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}_{\mathrm{i}}^{\mathrm{o}}$, where $\mathrm{x}_{\mathrm{i}}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture $p_{i}^{o}=$ pressure of $i^{\text {th }}$ gas in pure state
4 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}$, where $\mathrm{pi}=$ partial pressure of $\mathrm{i}^{\text {th }}$ gas $\mathrm{xi}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture
Explanation:
Dalton's law of partial pressures according to this law, the total pressure by a mixture of gases is equal to the sum of the partial pressures of each of the constituent gases. i.e. partial pressure of gas $=$ mole fraction of gas in gaseous mixture $\times$ Total pressure of gaseous mixture. $\begin{aligned} & \mathrm{P}_{1}=\mathrm{X}_{1} \mathrm{P} \\ & \mathrm{P}_{2}=\mathrm{X}_{2} \mathrm{P} \\ & \mathrm{P}_{3}=\mathrm{X}_{3} \mathrm{P} \end{aligned}$ $\therefore$ Total pressure $\mathrm{P}=\mathrm{P}_{1}+\mathrm{P}_{2}+\mathrm{P}_{3}$
NEET-17.06.2022
SOLUTIONS
277443
The osmotic pressure of a $5 \%$ (wt./vol) solution of cane sugar at $150^{\circ} \mathrm{C}$ is
277444
A $3 \mathrm{~mL}$ of solution was made by dissolving 20 mg of protein at $0^{0} \mathrm{C}$. The osmotic pressure of the resulting solution is 3.8 torr. The molecular weight of the protein is approximately (in g/mol)
277445
$\mathrm{pH}$ of a $0.1 \mathrm{M}$ monobasic acid is 2. Its osmotic pressure at a given temperature $T(K)$ is (Given that the effective concentration for osmotic pressure is $(1+\alpha) \cdot x$ concentration of acid: $\alpha$ is the dissociation factor)
277439
Which one is not correct mathematical equation for Dalton's law of partial pressure? Here $p=$ total pressure of gaseous mixture.
1 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}_{\mathrm{i}}^{\mathrm{o}}$, where $\mathrm{x}_{\mathrm{i}}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture $p_{i}^{o}=$ pressure of $i^{\text {th }}$ gas in pure state
4 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}$, where $\mathrm{pi}=$ partial pressure of $\mathrm{i}^{\text {th }}$ gas $\mathrm{xi}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture
Explanation:
Dalton's law of partial pressures according to this law, the total pressure by a mixture of gases is equal to the sum of the partial pressures of each of the constituent gases. i.e. partial pressure of gas $=$ mole fraction of gas in gaseous mixture $\times$ Total pressure of gaseous mixture. $\begin{aligned} & \mathrm{P}_{1}=\mathrm{X}_{1} \mathrm{P} \\ & \mathrm{P}_{2}=\mathrm{X}_{2} \mathrm{P} \\ & \mathrm{P}_{3}=\mathrm{X}_{3} \mathrm{P} \end{aligned}$ $\therefore$ Total pressure $\mathrm{P}=\mathrm{P}_{1}+\mathrm{P}_{2}+\mathrm{P}_{3}$
NEET-17.06.2022
SOLUTIONS
277443
The osmotic pressure of a $5 \%$ (wt./vol) solution of cane sugar at $150^{\circ} \mathrm{C}$ is
277444
A $3 \mathrm{~mL}$ of solution was made by dissolving 20 mg of protein at $0^{0} \mathrm{C}$. The osmotic pressure of the resulting solution is 3.8 torr. The molecular weight of the protein is approximately (in g/mol)
277445
$\mathrm{pH}$ of a $0.1 \mathrm{M}$ monobasic acid is 2. Its osmotic pressure at a given temperature $T(K)$ is (Given that the effective concentration for osmotic pressure is $(1+\alpha) \cdot x$ concentration of acid: $\alpha$ is the dissociation factor)
277439
Which one is not correct mathematical equation for Dalton's law of partial pressure? Here $p=$ total pressure of gaseous mixture.
1 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}_{\mathrm{i}}^{\mathrm{o}}$, where $\mathrm{x}_{\mathrm{i}}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture $p_{i}^{o}=$ pressure of $i^{\text {th }}$ gas in pure state
4 $\mathrm{p}_{\mathrm{i}}=\mathrm{x}_{\mathrm{i}} \mathrm{p}$, where $\mathrm{pi}=$ partial pressure of $\mathrm{i}^{\text {th }}$ gas $\mathrm{xi}=$ mole fraction of $\mathrm{i}^{\text {th }}$ gas in gaseous mixture
Explanation:
Dalton's law of partial pressures according to this law, the total pressure by a mixture of gases is equal to the sum of the partial pressures of each of the constituent gases. i.e. partial pressure of gas $=$ mole fraction of gas in gaseous mixture $\times$ Total pressure of gaseous mixture. $\begin{aligned} & \mathrm{P}_{1}=\mathrm{X}_{1} \mathrm{P} \\ & \mathrm{P}_{2}=\mathrm{X}_{2} \mathrm{P} \\ & \mathrm{P}_{3}=\mathrm{X}_{3} \mathrm{P} \end{aligned}$ $\therefore$ Total pressure $\mathrm{P}=\mathrm{P}_{1}+\mathrm{P}_{2}+\mathrm{P}_{3}$
NEET-17.06.2022
SOLUTIONS
277443
The osmotic pressure of a $5 \%$ (wt./vol) solution of cane sugar at $150^{\circ} \mathrm{C}$ is
277444
A $3 \mathrm{~mL}$ of solution was made by dissolving 20 mg of protein at $0^{0} \mathrm{C}$. The osmotic pressure of the resulting solution is 3.8 torr. The molecular weight of the protein is approximately (in g/mol)
277445
$\mathrm{pH}$ of a $0.1 \mathrm{M}$ monobasic acid is 2. Its osmotic pressure at a given temperature $T(K)$ is (Given that the effective concentration for osmotic pressure is $(1+\alpha) \cdot x$ concentration of acid: $\alpha$ is the dissociation factor)
