Practice Problem BUILD
Write the equation for the equilibrium that corresponds to each of the following reaction quotients:
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Chemistry
- 13 ut of Toluene, C₂Hs(9), is an important organic solvent and can be produced as represented by the following equilibrium equation. CH₁4(g) + energy C7Hs (g) + 3H₂(g) The equilibrium expression for this reaction equation is Select one: Kc = Kc = Kc = Kc = [C7Hs (g)]³[H₂(g)] [C7H14(g)] [C7H14(g)] [C7H8(g)]³[H₂(g)] [C7H8(g)][H₂(g)} [C7H₁4(g)] [C7H14(g)] [C7H8(g)][H₂(g)]³arrow_forwardThe equilibrium constant for the equilibrium, 3A+ 2B ↔ 2D + E, is 4.22 x 10-3 . What is the equilibrium constant for the equilibrium: D + (1/2)E ↔ (3/2)A + B? (a)237 (b)2.11×10-3 (c)15.4 (d)-2.11×10-3arrow_forwardAt 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_forward
- The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K. NH4I(S) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 7.23 L container at 673 K contains 2.31 mol of NH4I(s) and 0.237 mol of NH3(g), the partial pressure of HI(g) is atm. $ 4 Submit Answer F F4 % 5 T [Review Topics] [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining F5 G Cengage Learning | Cengage Technical Support A 6 MacBook Air ... Y H & 7 U J 8 ► 11 F8 ۔ 9 K Þ O ) –0 L F10 P 4) F11 Previous J + + 11 Next> Save and Exit 4) F12arrow_forward5. Dinitrogen pentoxide is added to an evacuated rigid container at 25°C. Given that the initial pressure is 1.00 atm and at equi- librium the pressure is 0.500 atm, determine the final pressure in the reaction vessel at equilibrium. 2N2O5(g) = 4NO2(g) + O2(8) (A) 0.750 atm (B) 1.00 atm (C) 1.25 atm (D) 1.75 atmarrow_forward2 NOBr(g) 2 NO(g) + Br,(g) AH = 16.1 kJ How does the equilibrium shift after the following stresses? d) Increase the container volume Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say e) Add a catalyst f) Add some N2 Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't sayarrow_forward
- A chemical equilibrium A ⇄ 2B has a forward rate constant, kf = 12 M –1 s–1, and a reverse rate constant, kr = 18 s–1. If the system has a concentration of [A] = 0.15 M at equilibrium, what is the concentration of B at equilibrium? (no scientific notation)arrow_forwardQ Search this course Reference Use the References to access importantv needed for this question. The equilibrium constant, K, for the following reaction is 1.20x102 at 500 K PCI5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.164 M PCI 4.43x10 M PCI3 and 4.43x10 M C2. What will be the concentrations of the three gases equilibrium has been reestablished, if 2.27x10 mol of Ch(g) is added to the flask? once [PCI5]= [PCI3]= М [Cl2] sturbing Equilibrium Concentrations (Qua... : This is group attempt 1 of 5 Next ack 1:33 PM 9/24/2019 up Xxarrow_forwardThe equilibrium constant for the following reaction is 6.50-10 at 298 2NOBrig)2NO(g) + Br₂(g) If an equilibrium mixture of the three gases in a 12.2 L container at 298K contains 0.343 mol of NOBrig) and 0.481 mol of NO, the equilibrium concentration of Brais [ Submit Answer 2 question attempts remainingarrow_forward
- 1 (a) N₂(g) + O₂(g) 2NO (g) AH298 + 180 kJ mol-¹ From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N2 (e) Adding a catalystarrow_forwardWhich of the following is at equilibrium? Select all that apply (a) The rate of the reverse reaction does not change b) The rate of the forward reaction is twice as fast as the rate of the reverse reaction. c) The concentrations of the reactants and products are equal. (d) The concentration of the reactants and the products do not change. (e) The rates of the forward and reverse reactions are equalarrow_forward) N2 (g) + 3H2 (g) NH3 (g) AH is negative From the given reaction at equilibrium above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of ammonia (b) Increasing pressure (c) Increasing the temperature (d) Adding a catalyst (e) Increasing the concentration of hydrogen will shift the equilibrium position to the left (State True or False)arrow_forward
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