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CHM 145 Lecture 10: CHM 145 2/7/17

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salmonwalrus328

15 Feb 2017

School

Oakland University

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Course

Professor

Charlene Hayden

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Document Summary

In an experiment, 1. 0 mol of n2o4 is placed in a 10. 0 l vessel and is allowed to react as described below. N2o4 (g) <===> 2no2 (g) kc = 4. 0 x 10-7 calculate the concentration of each species at equilibrium. = [no2]2 = [2x]2 = 4. 0 x 10-7. X2 = (4. 0 x 10-7) (. 10) = 1. 0 x 10-4. [no2]2 = 2 x 1. 0 x 10-4 = 2. 0 x 10-4 m. 0. 100-. 00010 = . 10m: the following reaction has an equilibrium constant, kc, equal to 3. 59 at 900oc. Ch4(g) + 2h2s (g) cs2 (g) + 4h2(g) For each of the following compositions, decide whether the reaction mixture is at equilibrium. If it is not, decide which direction the reaction will shift: [ch4]=1. 26m, [h2s]=1. 32m, [cs2]=1. 43m, [h2]=1. 12 m. [ch4][h2s]2 [1. 26][1. 32]2 2. 195: [ch4]=1. 25m, [h2s]=1. 52m, [cs2]=1. 15m, [h2]=1. 73 m. [cs2][h2]4 = [1. 15][1. 73]4 = 3. 57=3. 59 within experimental error. [ch4][h2s]2 [1. 25][1. 52]2: [ch4]=1. 20m, [h2s]=1. 31m, [cs2]=1. 15m, [h2]=1. 85 m.

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Related Questions

in an experiment, 1.0 mol of N₂O₄ isplaced in a 10.0 L vessel and is allowed to react as describedbelow.

N₂O₄ (g) <==> 2 NO₂(g)K_c= 4.0 * 10^-7

Calculate the concentration of each species at equilibrium.

The following data were obtained for the hypothetical reaction 2A + B rightarrow products. What is the overall order of this reaction? A0 3 B) 0 C) 1/2 D) 4 E) 1 The following reaction is investigated (assume an ideal gas mixture); 2N_2O(g) + N_2H_4(g) 3N_2(g) + 2H_2O(g) Initially there are 0.10 mol of N_2H_4, in = 10.0-L container. If there are 0.062 mol of N_2O at equilibrium, how many moles of N_2 are present at equilibrium? A) 1.9 times 10^-2 B) 5.7 times 10^-2 C) 1.1 times^10-5 D) 3.8 times 10^2 E) none of these For a certain second-order decomposition reaction, the rate is 0.40 mol/(L middot s) when the concentration of the reactant is 0.33 mol/L. What is the rate constant for this reaction? A) 1.21 L/(mol middot s) B) 0.40 L/(mol middot s) C) 0.27 L/(mol middot s) D) 0.83 L/(mol middot s) E) 3.7 L/(mol middot s) Exactly 1.0 mol N-2O_4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N_2O_4(g) 2NO-2(g). IF at equilibrium the N_2O_4 is 38.0% dissociated, what is the value of the equilibrium constant, K_c, for the reaction under these conditions? A) 0.93 B) 1.23 C) 0.58 D) 1.1 E) 0.23 A 35.0-L vessel at 700 K initially contains HI(g) at a pressure of 3.60 atm; at equilibrium, it is found that the partial pressure of H_2(g) is 0.348 atm. What is the partial pressure of HI(g) at equilibrium? 2HI(g) H_2(g) + I_2(g) A) 0.348 atm B) 3.25 atm C) 3.60 atm D) 3.95 atm E) 2.90 atm For the hypothetical reaction 2A + B rightarrow 2C + D, the initial rate of disappearance of A is 2.0 times 10^-2 mol/(L middot s). What is the initial rate of disappearance of B? A) 1.4 times 10^-1 mol/(L middot s) B) 1.0 times 10^-2 mol/(L middot s) C) 8.0 times 10^-2 mol/(L middot) D) 4.0 times 10^-4 mol/(L middot s) E) 1.4 times 10^-2 mol/(L middot s) In an experiment, 0.44 mol H_2 and 0.44 mol I_2 are mixed in a 1.00 - L container, and the reaction forms HI. If K_c = 49, for this reaction, what is the equilibrium concentration of HI? I_2(g) + H_2(g) 2HI(g) A) 0.059 M B) 0.77 M C) 0.68 M D) 0.110 M E) 0.85 M If K_c = 0.132 for A_2 + 2B 2AB, what is the value of K_c for the reaction 4AB 2A_2 + 4B? A) 57.4 B) -0.132 C) 0.132 D) 3.79 E) 0.264

Please answer but also explain all of them! Thank you!