Starting with 0.133 mol X2 and 0.199 mol Y2 in a 5.00 L container, calculate the partial pressure of each species at equilibrium.
Question
Starting with 0.133 mol X2 and 0.199 mol Y2 in a 5.00 L container, calculate the partial pressure of each species at equilibrium.
Solution
To calculate the partial pressure of each species at equilibrium, we need to use the ideal gas law equation, which is PV = nRT. Here, P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. However, the temperature is not given in the problem, so we'll assume that the temperature remains constant.
Step 1: Calculate the total moles of gas The total moles of gas is the sum of the moles of X2 and Y2, which is 0.133 mol
Similar Questions
If the air in a container contains 92.94% oxygen, what is the partial pressure of oxygen in the container if the total pressure 28.84 atm?
2 H2O2(l) 2 H2O(g) + O2(g) Decompose 0.11 g of H2O2 in a flask with a volume of 2500.0 mL. What is the pressure of O2 at 25 oC? Of H2O?
How many moles of gas (to 1 decimal place, input value only), are contained in a 54.25 L vessel at a pressure of 173.6 kPa and temperature of 0.2 °C?
A diver uses an air tank that contains 75.7 % nitrogen. Determine the partial pressure of the nitrogen at 17.1 m.
At 20 l flash at 500 Kelvin ab gas 4 ATM the equilibrium passed a pressure of a 20.387 find the equilibrium pressure of a b
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.