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Consider the equilibrium A<sub>(g)</sub> + B<sub>(g)</sub> = AB<sub>(g)</sub>. When the partial pressure of A is 10<sup>-2</sup> atm, the partial pressure of B is 10<sup>-3</sup> atm and the partial pressure of AB is 1 atm, the equilibrium constant 'K' is

Correct Answer: 10<sup>5</sup> atm<sup>-1</sup>

Consider the equilibrium A(g) + B(g) = AB(g). When the partial pressure of A is 10-2 atm; the partial pressure of B is 10-3 atm and the partial pressure of AB is 1 atm; the equilibrium constant K is

What is the total pressure of a system having 25% CO2 with 4 atm partial pressure and 30% O2 with 10 atm partial pressure, and 45% SO2 with partial pressure 20 atm?

What is the fraction of a gas in a system at partial pressure 1 atm, if the 0.1 fraction of the same gas is at partial pressure 2 atm and 0.2 fraction at partial pressure 4 atm (Use Freundlich Isotherm)?

What is the fraction of a gas in a system at partial pressure 1 atm, if the 0.2 fraction of the same gas is at partial pressure 4 atm and 0.4 fraction at partial pressure 8 atm (Use Freundlich Isotherm)?

What is the fraction of a gas in a system at partial pressure 3 atm, if the 0.2 fraction of the same gas is at partial pressure 4 atm and 0.3 fraction at partial pressure 6 atm (Use Freundlich Isotherm)?

The highest pressure gas of a mixture has partial pressure p, the partial pressure of other gases decreases by factor of 2n-1, the partial pressure of second gases decreases by a factor of 2, partial pressure of third gas increases by 4, and so on, if the total pressure of gas mixture is 31p/16, how many gases are present in the mixture?

If the initial partial pressure of Cl2 in container A is 1.0 atm and the initial partial pressure of H2O is also 1.0 atm, what will be the pressure at equilibrium?

If u (x, y, z, t) = f(x + iβy - vt) + g(x - iβy - vt), where f and g are arbitrary and twice differentiable functions, is a solution of the wave equation $$\frac{{\partial {u^2}}}{{\partial {x^2}}} = \frac{{{\partial ^2}u}}{{\partial {y^2}}} = \frac{1}{{{c^2}}}\frac{{{\partial ^2}u}}{{\partial {t^2}}}$$     then β is

The Henry’s law constant for O2 in water at 25°C is 1.27×10−3M/atm and the mole fraction of O2 in the atmosphere is 0.21. Calculate the solubility of O2 in water at 25°C at an atmospheric pressure of 1.00 atm. Strategy: ▪ Use Dalton’s law of partial pressures to calculate the partial pressure of oxygen. ▪ Use Henry’s law to calculate the solubility, expressed as the concentration of dissolved gas.

What is the total pressure of a system having 40% O2 with 5 atm partial pressure and 60% N2 with 10 atm partial pressure?