Three bulbs containing 3 gasses at varying pressures are connected by stopcocks in the apparatus displayed. What happens to the system's pressure when the stopcocks are opened? Assume that the temperature stays constant and that the lines connecting the bulbs have a volume of zero.

67.5% SO₂ and 32.5% CO₂ make up a special gas chamber. At 839 atm total pressure, what is each gas's partial pressure in atmospheres?

Consider the reaction below: 

CO(g) + H₂O(g) ↔ CO₂(g) + H₂(g) 

An equilibrium mixture of 38.9 g CO, 25.0 g H₂O, 26.9 g CO_2, and 1.23 g H₂ is kept in a 2.00 L container at 1260 K. Calculate the total pressure of the mixture.

Calculate the partial pressure of NO and Kr in air at 1.23 bar if their mole fractions are 5.00 x10^-7 and 1.14x10^-6 respectively.

The total pressure of an unknown gas and water in a closed container is 708.3 torr at 150 °C. Determine the partial pressure of the unknown gas after condensing water at 6°C if their mol ratio was 4:3. (Assume that volume is constant)

A 285 mL flask contains a mixture of CO, CO₂, and O₂ at 15°C. What is the partial pressure of O₂ if the total pressure is 795 torr, the CO has a partial pressure of 265 torr and the CO₂ has a partial pressure of 355 torr?

A CO₂-SO₂-H₂O mixture was collected in a 21.0-L steel tank until the pressure reaches 861.4 torr at 58.0°C. 

(a) Calculate the moles of gas collected. 

(b) What is the partial pressure (torr) of SO₂ if its concentration in the mixture is 1.83×10³ parts per million (ppmv)? (Hint: ppmv = volume of component/volume of mixture) x 10⁶.)