Short Answer TypeHow is Dalton's law of partial pressures useful in calculating the pressure of a dry gas?
Long Answer Type300 mL of a gas A at a pressure of 600 mm is mixed with 200mL of another gas B at a pressure of 700 mm in a vessel of 2-litre capacity. What will be the total pressure of the resulting mixture, if the temperature is kept constant?
Let the partial pressure of the gases A and B be represented by PAÂ and PBrespectively.
(i) Partial pressure of gas A in 2 litre flask:
  V1 = 300 mL;    P2 = 600 mm
  V2 = 2 L = 2 x 1000 = 2000 mL;  PA = ?
According to Boyle's law, Â P1V1 = P2V2
i.e. Â 600 x 300 = PA x 2000
(ii) Partial pressure of gas B in 2 litre flask:
    V1 = 200 mL,  P1 = 700 mL
    V2 = 2 litre = 2 x 1000 = 2000 mL
    PB = ?
According to Boyle's law,
       P1V1 = P2V2
i.e. Â Â 700 x 200 = PB X 2000
Â
What will be the pressure of the gaseous mixture when 0.5 L of H2 at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C?Â
A neon-dioxygen mixture contains 70.6 g dioxygen and 167·5 g neon. If pressure of the mixture of gases in the cylinder is 25 bar, what is the partial pressure of dioxygen and neon in the mixture?Â
Short Answer TypeA mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.Â
Long Answer TypeCalculate the total pressure in a mixture of 8g of dioxygen and 4g of dihydrogen confined in a vessel of 1 dm3 at 27°C. R = 0·083 bar dm3 k–1 mol–1.Â
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