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Practice Problem 
ATTEMPT
Write equilibrium expressions for each of the following reactions:
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Chapter 15 Solutions
Chemistry
- Question plzarrow_forward9:29 Question 14 of 16 Submit Which of the following is the correct expression for the pressure based equilibrium constant for the reaction: 2 NO (g) + Br2 (1) 2 NOBR (g) PRo PBr2 A) Kp NOBR B) Kp p2 ΝOr NOB C) Kp PNO D) Kp = PROBT A) see problem image B) see problem image C) see problem image Periodic Tablearrow_forwardPractice chemistry questionarrow_forward
- At a certain temperature, the value of the equilibrium constant, K, for the reaction represented below is 2.0 x 105. What is the value of K for the reverse reaction at the same temperature? H2(g) + Br2(g) = 2HBr(g) (A) -2.0 x 10-5 (B) 5.0 x 10-6 (C) 2.0 x 10-5 (D) 5.0 x 10-5arrow_forwardPractice Exercise At 1280°C the equilibrium constant (K.) for the reaction Br2(g) = 2Br(g) is 1.1 x 10-3. If the initial concentrations are [Br2] 6.3 x 10-2 M and [Br] = 1.2 × 10-2 M, calculate the concentrations of these species at equilibrium.arrow_forwardCheck Your Understanding In each of the following, determine the direction in which the equilibrium will shift in response to the indicated stress. (a) N2 (g) + 3 H2 (g) 2 2 NH3 (g); pressure is decreased Answer + Shift toward reactants (b) CO2(g)+ H2 (g) 2 CO(g) +H2O(g); pressure is increased Answer no changearrow_forward
- Given a K value of 4.6 X 10-12, would you expect a nearly complete reaction at equilibrium? yes no insufficient informationarrow_forwardHere are equilibrium constants for several reactions. Which of them favor the formation of products, and which favor the formation of reactants? (a) 4.5 X 10-8 (b) 32 (c) 4.5 (d) 3.0 x 10-7 (e) 0.0032arrow_forwardWhat is the relationship of 5 points equilibrium constants for the following two reactions? (1) 2 NO,(g) > N,0,(g); K, (2) N,0,(g) > 2 NO,(g) K2 (a) K,= 1/ K2 O Option 1arrow_forward
- Question attachedarrow_forwardPractice Exercise At 1280°C the equilibrium constant (K) for the reaction Br2(g) 2Br(g) is 1.1 x 10 . If the initial concentrations are [Br2] 102 M, calculate the concentrations of these species at equilibrium. 6.3 x 10 2 M and [Br] = 1.2 X !!arrow_forwardNonearrow_forward
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