The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 4. What is the value of Kp? (2023)
Practice Questions
1 question
Q1
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 4. What is the value of Kp? (2023)
4
16
0.25
0.0625
Kp can be calculated from Kc using the relation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas. Here, Δn = 2 - 3 = -1, so Kp = Kc(0.0821T)^(-1). Assuming standard conditions, Kp = 4 * (1/RT) = 16.
Questions & Step-by-step Solutions
1 item
Q
Q: The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 4. What is the value of Kp? (2023)
Solution: Kp can be calculated from Kc using the relation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas. Here, Δn = 2 - 3 = -1, so Kp = Kc(0.0821T)^(-1). Assuming standard conditions, Kp = 4 * (1/RT) = 16.
Steps: 10
Step 1: Identify the given equilibrium constant Kc, which is 4.
Step 2: Write down the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g).
Step 3: Determine the change in moles of gas (Δn). Count the moles of gas on the reactant side (3 moles: 2 from SO2 and 1 from O2) and the product side (2 moles from SO3).
Step 4: Calculate Δn: Δn = moles of products - moles of reactants = 2 - 3 = -1.
Step 5: Use the formula Kp = Kc(RT)^(Δn). Here, R is the gas constant (0.0821 L·atm/(K·mol)) and T is the temperature in Kelvin. Assume standard conditions (T = 298 K).
Step 6: Substitute the values into the formula: Kp = 4 * (0.0821 * 298)^(-1).
Step 7: Calculate (0.0821 * 298) to find the value of RT.
Step 8: Take the reciprocal of RT to find (RT)^(-1).
