N2O4 (g) <------> 2 NO2 (g)
I (M) 0.20 0
E (M) 0.20 -x 2x
Kc = [NO2]2/[N2O4]
1.2 = (2x)2/(0.20-x)
4x2 + 1.2 x - 0.24 = 0
x = 0.137 M
[NO2] = 2x = 0.274 M
[N2O4] = 0.20-x = 0.063 M
N20 (9) 5 2 NO2(g) A reaction mixture at 550 "C initially contains [N,01] = 0.20...
Consider the following reaction: NO2(g) + N(graphite) ⇌ 2 NO(g) A reaction mixture initially contains 0.86 atm NO2 and 0.42 atm NO. Determine the equilibrium pressure of NO if Kp for the reaction is 3.25
Question 2 (5 points) Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) = 503(9) + NO(g) Kc = 0.33 A reaction mixture initially contains 0.61 M SO2, 0.10 M NO2, 0.16 M SO, and 0.23 M NO. Which of the following statements is TRUE? The reaction is already at equilibrium The reaction will proceed in the direction of products to reach equilibrium The reaction quotient is larger than the equilibrium constant The rates of the forward and...
Part A a mixture contains A, B, and C in the following concentrations: [A] = .550 M, [B] = 1.10 M, and [C] = .650 M. The following reaction occurs and equilibrium is established. what is Kc? myct/itemView?assignment ProblemID=143011484&offset=next Mrs. Graves AP Chemistry Chloe & © 55: Calculating the Equilibrium Constant and the Reaction Quotient ③ 3 of 5 Review Constants Periodic Table Part A A mixture initially contains A, B, and occurs and equilibrium is established: in the following...
Dinitrogen tetroxide decomposes to produce nitrogen dioxide: N204 (9) - 2 NO2 (g) Calculate the equilibrium constant for the reaction given the equilibrium concentrations at 100°C: [N204] = 0.800 M and [NO2] = 0.400 M A. 5.00 OB.0.200 OC. 0.500 OD.2.00
16. Consider the equilibrium, 2HBr(9) H,(g)+Br (g). If 2.0 M HBr(g) is placed in a container, then at equilibrium, the HBr(g) concentration is 1.4 M. Therefore, the equilibrium constant, Kc, for this reaction is approximately: (A) 0.046 (B) 0.064 (C) 0.21 (D) 0.26 07. For the reaction, N,O,(9) >2NO2(g), Ko = 0.40 at a certain temperature in an equilibrium mixture of the two gases, the concentration of N204 is 0.50 M. The concentration of NO2 in this mixture is approximately:...
please show all steps. find equiibrium concentration of N2O4 and NO2 Consider the following reaction: N2O4(g) = 2NO2(g), K = 0.36 at 2000°C The reaction mixture initially contains only the reactant, (N204] = 0.0220M , and no NO2.
Question 2 (5 points) ✓ Saved Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) = SO2(g) + NO(g) K = 0.33 A reaction mixture initially contains 0.61 M SO2, 0.10 M NO2, 0.16 M SO3 and 0.23 M NO. Which of the following statements is TRUE? The reaction is already at equilibrium The reaction will proceed in the direction of reactants to reach equilibrium The rates of the forward and backward reactions are initially equal The reaction...
Consider the following reaction: COCl2(g) = CO(g) + Cl2(8) A reaction mixture initially contains 1.6 M COC12. Determine the equilibrium concentrations of COCI, CO, and Cl2 if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. Use x is small approximation. Show Q Validity check [Cl2] = [CO]= [COCI2] = Calculate the reaction quotient, Q A % Validity Check A Calculate the A/ equilibrium...
Consider the following reaction: N2O4(g)⇌2NO2(g),Kc=0.36 at 2000∘C The reaction mixture initially contains only the reactant, [N2O4]=0.0300M , and no NO2. Find the equilibrium concentration of N2O4. Find the equilibrium concentration of NO2.
Consider the following reaction: CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)A reaction mixture initially contains 0.50 M CH4 and 0.75 M H2S. If the equilibrium concentration of CS2 is 0.15 M, what is the equilibrium constant (Kc) for the reaction.Hint: You might need an I.C.E. Table for this one. please show work