(Set 1) Practice Problems in Equilibrium Part A: Finding K A(g) + 3 B(g) 2 C(g) 1. Initially [A] -0.52 M and [B] - 1.82 M. At equilibrium (A) - 0.22 M. Find K. 2. [C] -1.55 M, and (C) -0.044 M. Determine the value of K. 3. Initially [C] -0.00455 M; at equilibrium (B) - 0.00035. What is K? 20,() = 3 02(8) 4. 10.1-0.5 M, and [O:) -0.5 M. What is the value of K? 5. What is...
2 NO(g) 근 N2(g) + O2(g) 9. [NO].-0.50 M and [N2]i-0.030 M. If K = 7000, find [NOLq.
What is the ΔS° at 298 K for the following reaction? 2 O3(G) ---- 3 O2(G) Substance ΔS° (J/mol·K) O2(g) 205.0 O3(g) 238.8
Question 29 (1 point) Consider the decomposition reaction 2NO(g) + N2(g) + O2(g). When 0.20 M sample of NO(g) was decomposed at a given temperature, the equilibrium concentration of N2 was 0.040 M. What was the equilibrium concentration of NO(g)? 0.12 M 0.040 M 0.24 M 0.080 M Previous Page Next Page Page 29 of 30
Assume the reaction 3 O2(g) <===> 2 O3(g) (Delta H° =285 kJ/mol) is at equilibrium. What effect will each of the following have (explain each)? a) adding more O2 b) adding more O3 c) removing O3 d) increasing pressure in the container e) adding an inert gas f) increasing the temperature in the container
2 NO (g) equilibrium arrow N2 (g) + O2 (g) Initially, 0.75 M NO is placed in a reaction vessel and the reaction is allowed to reach equilibrium. If the equilibrium constant for this reaction is 0.463, what is the equilibrium concentration of NO?
Be sure to answer all parts. A) Calculate Kp for the following equilibrium: 3 O2(g) ⇌ 2 O3(g) Kc =1.8 × 10 −56 at 450 K __× 10__ B) Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium, [NH3] = 0.0233 M, [N2] = 0.119 M, and [H2] = 0.369 M. Calculate Kc for the reaction at this temperature. Kc = __
For the following reaction 3 O2 (g) → 2 O3 (g) ΔH = +286 kJ What is the ΔH when 16.0 g of O3 are produced
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
Part A N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 Part B C(s)+O2(g)⇌CO2(g) K=[CO2][O2] K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s)+H2O(g)+heat⇌CO(g)+H2(g) Part C What effect does each of the following changes have on the equilibrium? Drag the appropriate stresses to their respective bins. add H2O, Add heat, lower temperature, remove CO Categories: Equilibrium shifts to products, Equilibrium shifts to reactants, Equilibrium doesn't shift