Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
Consider the Haber process:
3 H2(g) + N2(g) 2 NH3(g); Kc = 63.2 at 272°C,
At one point in the reaction, a sample of the reaction mixture was analyzed for contents: [N2] =
6.00 10–1 M, [H2] = 1.25 M and [NH3] = 3.75 10–2 M. Which of the statements is correct?
A. the reaction is at equilibrium
B. the reaction is moving in reverse to achieve equilibrium
C. the reaction is moving forward to achieve equilibrium
D. it is impossible to tell from the information given
E. none of the above
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- 4arrow_forwardFor the reaction, 2NH3(g)--> <---3H2 (g)+ N2 (g) the equillibrium concentrations were found to be [NH3 ]=0.250 M, [H2 ]=0.540 M, and [N2 ]= 0.750 M. What is the equilibrium constant for this reaction? Kc=?arrow_forwardDuring an experiment, O.257 mol of H2 and 0.257 mol of I2 were placed into a 1.28 liter vessel where the reaction H2(g) + 12(g) 2 2HI(g) came to equilibrium. For this reaction, Kc = 49.5 at the temperature of the experiment. What were the equilibrium concentrations of H2, 12, and HI? [H2] = M %3D [12] = M [HI] = i Marrow_forward
- At 460 °C, the reaction * NO(g) + SO3(g) SO2(g) + NO2(g) has Kc = 85.0. Suppose 0.109 mol of SO2, 0.0612 mol of NO2, 0.0755 mol of NO, and 0.118 mol SO3 are placed in a 10.0 L container at that temperature. What will the concentrations of all the gases be when the system reaches equilibrium? %3D [SO2) = M i [NO2] = M %3D [NO] = i M [SO3] = i Marrow_forwardA mixture containing an initial concentration of 0.1590 M for H2 and 0.1329 M for I2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HI?H2(g) + I2(g) ↔ 2HI(g) Kc = 48.7000arrow_forwardNeed helparrow_forward
- Hh.53.arrow_forward7 4 (a) Calculate the value of Kc for the reaction: PC15 (2) PC13 (g) + Cl2 (g) AH = Positive Given that when 8.4 mol of PCls (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PCls (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (1) Increasing temperature (ii) Lowering the concentration of chlorine (Cl2) (iii) Addition of a catalystarrow_forward(Q96) The equilibrium constant with respect to concentration (K) fer the reaction between nitrogen monoxide and oxygen gas to produce nitrogen diexide is 5.4 x 1013 at 25 C. What is the value ef the equilibrium constant with respect to partial pressures (Ke) under these same eenditiens? (2 sf) O 2.2 x 10^12 O5.4 x 10A13 1.3 x 19A15 @ 11x 1014 2.2x10 10arrow_forward
- Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N2 and Og (from air). N2 (9) + O2(9) - 2NO(9) The equilibrium constant (K.) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.082 mol N, and 0.026 mol O2 per liter, what is the concentration of NO? Concentration = Marrow_forward6. At 27°C, K=2.6 X 105 for the reaction 2 NH3 (g) > N2 (g) + 3 H2 (g) Calculate the value of K for the following: a.) NH3(g) > ½ N2(g) + 3/2 H;(g) b.) N2(g) + 3 H2(g) 2 NH3(g)arrow_forward
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