319376 How many grams of \(\mathrm{CO}_{2}\) gas is dissolved in a \(1 \mathrm{~L}\) bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at \(25^{\circ} \mathrm{C}\). Given \(\mathrm{K}_{\mathrm{H}}\) of \(\mathrm{CO}_{2}\) water \(=29.76 \mathrm{~atm} . \mathrm{L} / \mathrm{mol}\) at \(25^{\circ} \mathrm{C}\)

319377 According to Henry’s law ‘the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution’. For different gases the correct statement about Henry’s constant is

319378 Henry's law constant for \(\mathrm{CH}_{3} \mathrm{Br}\) is
\(0.16 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{bar}^{-1}\) at \(298 \mathrm{~K}\). What pressure is required to have solubility of \({\text{0}}{\text{.08}}{\mkern 1mu} {\text{mol}}{\mkern 1mu} {{\text{L}}^{{\text{ - 1}}}}{\text{?}}\)

319379 The law which indicates the relationship between solubility of a gas in liquid and pressure is :

319376 How many grams of \(\mathrm{CO}_{2}\) gas is dissolved in a \(1 \mathrm{~L}\) bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at \(25^{\circ} \mathrm{C}\). Given \(\mathrm{K}_{\mathrm{H}}\) of \(\mathrm{CO}_{2}\) water \(=29.76 \mathrm{~atm} . \mathrm{L} / \mathrm{mol}\) at \(25^{\circ} \mathrm{C}\)

319377 According to Henry’s law ‘the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution’. For different gases the correct statement about Henry’s constant is

319378 Henry's law constant for \(\mathrm{CH}_{3} \mathrm{Br}\) is
\(0.16 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{bar}^{-1}\) at \(298 \mathrm{~K}\). What pressure is required to have solubility of \({\text{0}}{\text{.08}}{\mkern 1mu} {\text{mol}}{\mkern 1mu} {{\text{L}}^{{\text{ - 1}}}}{\text{?}}\)

319379 The law which indicates the relationship between solubility of a gas in liquid and pressure is :

319376 How many grams of \(\mathrm{CO}_{2}\) gas is dissolved in a \(1 \mathrm{~L}\) bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at \(25^{\circ} \mathrm{C}\). Given \(\mathrm{K}_{\mathrm{H}}\) of \(\mathrm{CO}_{2}\) water \(=29.76 \mathrm{~atm} . \mathrm{L} / \mathrm{mol}\) at \(25^{\circ} \mathrm{C}\)

319377 According to Henry’s law ‘the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution’. For different gases the correct statement about Henry’s constant is

319378 Henry's law constant for \(\mathrm{CH}_{3} \mathrm{Br}\) is
\(0.16 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{bar}^{-1}\) at \(298 \mathrm{~K}\). What pressure is required to have solubility of \({\text{0}}{\text{.08}}{\mkern 1mu} {\text{mol}}{\mkern 1mu} {{\text{L}}^{{\text{ - 1}}}}{\text{?}}\)

319379 The law which indicates the relationship between solubility of a gas in liquid and pressure is :

319376 How many grams of \(\mathrm{CO}_{2}\) gas is dissolved in a \(1 \mathrm{~L}\) bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at \(25^{\circ} \mathrm{C}\). Given \(\mathrm{K}_{\mathrm{H}}\) of \(\mathrm{CO}_{2}\) water \(=29.76 \mathrm{~atm} . \mathrm{L} / \mathrm{mol}\) at \(25^{\circ} \mathrm{C}\)

319377 According to Henry’s law ‘the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution’. For different gases the correct statement about Henry’s constant is

319378 Henry's law constant for \(\mathrm{CH}_{3} \mathrm{Br}\) is
\(0.16 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{bar}^{-1}\) at \(298 \mathrm{~K}\). What pressure is required to have solubility of \({\text{0}}{\text{.08}}{\mkern 1mu} {\text{mol}}{\mkern 1mu} {{\text{L}}^{{\text{ - 1}}}}{\text{?}}\)

319379 The law which indicates the relationship between solubility of a gas in liquid and pressure is :