completed so far. It does not indicate completia Ret 2.0-x 0.50 2x 0 1.0 1.0+2x X X 0.50+x 2.0-2x Concentration (M) 2HI(g) Halg) 12lg) Initial 2.0 0 0 - 2x Change 2.0-x X Equilibrium Next> 9 of 24 < Prev Retur Fill in the equilibrium table for the reaction of HI to form H2 and ksub>2. (Pool: 2 of 3) Fill in the equilibrium table for the reaction of HI(d) to form H2(g) and I2(g Initial Conditions: A 1.0-L vessel is charged with 2.0 mol HI(g) at 100°C. 0.50-x 0.50-2x 0.50 2x 1.0 x 20 +2x 1.0 2x 1.0-x x -2x 2.0 x 0.50 2x 0 1.0 0.50+x 2.0-2x 1.0+2x X x 12lg) 2HI(g) H2(g) + Concentration (M) 0 2.0 Initial Next > 9 of 24 < Prev

completed so far. It does not indicate completia Ret 2.0-x 0.50 2x 0 1.0 1.0+2x X X 0.50+x 2.0-2x Concentration (M) 2HI(g) Halg) 12lg) Initial 2.0 0 0 - 2x Change 2.0-x X Equilibrium Next> 9 of 24 < Prev Retur Fill in the equilibrium table for the reaction of HI to form H2 and ksub>2. (Pool: 2 of 3) Fill in the equilibrium table for the reaction of HI(d) to form H2(g) and I2(g Initial Conditions: A 1.0-L vessel is charged with 2.0 mol HI(g) at 100°C. 0.50-x 0.50-2x 0.50 2x 1.0 x 20 +2x 1.0 2x 1.0-x x -2x 2.0 x 0.50 2x 0 1.0 0.50+x 2.0-2x 1.0+2x X x 12lg) 2HI(g) H2(g) + Concentration (M) 0 2.0 Initial Next > 9 of 24 < Prev

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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6. A 3.75-L vessel contains 0.444 mol SO3, 0,632 mol O2, and 2.125 mol SO2 at 230°C in an equilibrium mixture. Calculate the value of Kc at 230°C. (1 2SO2(g) + O2 (g) 2SO3 (9)
Consider the following system at equilibrium where Kc = 154 and H° = -16.1 kJ/mol at 298 K. 2 NO (g) + Br2 (g) 2 NOBr (g) The production of NOBr (g) is favored by:Indicate True (T) or False (F) for each of the following: ___decreasing the temperature. ___decreasing the pressure (by changing the volume). ___decreasing the volume. ___removing NOBr . ___adding Br2 .
At a certain temperature, the ?p for the decomposition of H2S is 0.770. H2S(g)↽−−⇀H2(g) + S(g) Initially, only H2S is present at a pressure of 0.268 bar in a closed container. What is the total pressure in the container at equilibrium? Ptotal= bar
Consider the following equilibrium: N₂(g) + 3H₂(g)2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 9.24 atm of ammonia system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this S
As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
Consider the following system at equilibrium where AH = 268 kJ and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) NH3(g) + HCl(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: decreasing the pressure (by changing the volume): increasing the volume: adding NH4Cl: adding HCl:
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if Kc and Qc are within 5% of each other.) (a.) 2 SO3(g) 2 SO2(g) + O2(g) Pi(SO3) = 0.100 atm, Pi(SO2) = 1.10 atm, Pi(O2) = 1.20 atm, Kp = 5.5 atm What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT? (b.) 2 NO(g) + Cl2(g) 2 NOCl(g) Pi(NO) = 1.25 atm, Pi(Cl2) = 1.25 atm, Pi(NOCl) = 0 atm, Kp = 3.1 ✕ 103 What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT? (c.) N2(g) + O2(g) 2 NO(g) [N2]i = 0.120 M, [O2]i = 0.240 M, [NO]i = 1.20 M, Kc = 0.050 What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT?
Question 15 of 16 Submit Consider the reaction below: 2 SO3(g) =2 SO2(g) + O2(g) The Kp is 1.81 × 10-5 at 350.0°C. Calculate Kc at the same temperature. (R = 0.08314 L·bar/ mol · K.) 1 2 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources LO
The reaction mixture below contains 0.112 atm of H2, 0.077 atm of S2, and 0.224 atm of H2S. 2 H2S(g) 2 H2(g) + S2(g) K, = 2.4x104 at a particular temperature. Based on the information provided, select the correct relationship. O Q > K; the reaction will proceed to form more H2S(g). O More experimental data are always needed to answer a question like this. OQ < K; the reaction will proceed to form more products. OQ= K; the reaction is at equilibrium and no change is expected.