Calculate P [NO]eq, if P [NOCl]eq = 0.33 atm, P [Cl2]eq = 0.50 atm, and Kp = 1.9 x 10-2. 2...
3. Calculate P [NO]eq, if P [NOCl]eq = 0.60 atm, P [Cl2]eq = 1.50 atm, and Kp = 3.9 × 10-2. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)
9. Which of the following acids is the WEAKEST? The acid is followed by its Ka value. A) HC2H302, 1.8 x 10-5 B) HIO, 2.3 x 10-11 C) HBrO, 2.3 x 10-9 D) HCIO, 2.9 x 10-8 E) C6H5CO2H, 6.3 x 10-5 10. Calculate P [NO]eq, if P [NOCIJeg = 0.33 atm, P [Cl2leq = 0.50 atm, and Kp = 1.9 x 10-2 2 NOCI(g) = 2 NO(g) + Cl2(g) A) 1.7 atm B) 0.0042 atm C) 0.30 atm D)...
2 NOCl(g) ⇄ 2 NO(g) + Cl2(g) Kp = 7.2× 10-6 1.50 atm of NOCl(g) is placed in a container and the system is allowed to reach equilibrium. Calculate the equilibrium pressure of Cl2(g) at equilibrium. 4.8 × 10-2 atm 8.5 × 10-3 atm 3.2 × 10-2 atm 2.4 × 10-2 atm 1.6 × 10-2 atm
Consider the following reaction: 2NO(g) + 12(g) = 2NOI() Kp = 1.6 x 10-5 Calculate the pressure of NOI (g) at equilibrium if initial pressures are 0.50 atm of NO(g) and 0.30 atm of 12(g) A B. C. D. E. 1.1 * 10-3 atm 7.2 x 10-4 atm 3.6 x 10-4 atm 1.8 * 10-3 atm 5.9 ~ 10-3 atm
0.0950 atm, PC120.171 atm, and PNOCI QUESTION 14 What is the equilibrium constant, Kp. for the reaction below if the equilibrium partial pressures are PNO 0.280 atm? 2 NO(g) + Cl2 (8) 2 NOCI (g) 4. 4.55 x 10-3 5.5.80 x 10-2 17.2 d. 50.8 e 1.97 x 10-2
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answer the question 1) Which of the following statements is FALSE? A) When K<< 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent. B) K>> implies that the reaction is very fast at producing products. When K>>> 1, the forward reaction is favored and essentially goes to completion. D) When K-1, neither the forward or reverse reaction is strongly favored,...
CO(g) + Cl2(g) <==-=> COCI2(8) AH = 58 kJ Determine Kp at 500°C if the pressure is in atm and Kc is 5.55 x 1010 A 5.82 x 10-5 B 2.28 x 1012 5.30 x 1025 1.35 x 10° E 8.75 x 108
NO2(g) ⇌ N2O4(g) Kp = 11.3 at 25oC (a) Calculate G if the P(NO2) = 0.29 atm, and P(N2O4) = 1.6 atm. (b) Predict the direction in which the reaction will shift to reach equilibrium. Explain how you determined this. (c) Once equilibrium is reached are there more reactants or products present. Explain how you determined this.
Consider the following equilibrium: 2NOCl(g) ⇌ 2 NO(g) + Cl2(g) Kc = 1.6 x 10-5 1.00 mole of pure NOCl and 1.00 mole of pure Cl2 are placed in a 1.00 L container. Calculate the equilibrium concentration of NO(g)
The equilibrium constant Kp for the reaction CC, (g) 근 C(s) + 2 Cl2 (g) at 700°C is 0.73. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 2.60 atm at 700c. Pressure- atm Try Another Version 4 item attempts remaining At a particular temperature, K = 2.0 × 10-6 for the reaction 2 CO (g) + O2 (g) 2 CO2 (g) If 2.5 moles of CO2 is initially placed into a 5.0-L vessel,...