PRACTICE PROBLEMS:1. The equilibrium 2 NOe) + Clle) 2 NOCI(g) is established at 500 K. An equilibrium mixtureor the three gases has partial pressures of 0.095 atm, 0.171 atm and 0.28 atm for NO, Cl2 andNOCI, respectively. Calculate the Kp for this reaction at 500 K.2. Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PC13(2) +Cl2(8) PCIS(g). A gas vessel is charged with a mixture of PCI3 and Cl2 which is allowed toequilibrate at 450 K. At equilibrium, the partial pressures of the three gases are What is thevalue of Kp at this temperature?3. A mixture of 0.2000 mol of CO,, 0.1000 mol of H, and 0.1600 mol of H20 is placed in a 2.000-Lvessel at 226 °C. The following equilibrium is established: CO2(e) + H2(g) =CO(8) + H2O(g)-Calculate the initial partial pressures of CO2, H2 and H2O.b. At equilibrium, . Calculate the equilibrium partial pressures of CO2, H2 and CO.Calculate K, for the reaction.a.С.

MS: 1. The equilibrium 2 NO(8) + Cl2te) = 2 NOCI(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm and 0.28 atm for NO, Cl2 and NOCI, respectively. Calculate the Kp for this reaction at 500 K. 2. Phospho

MS: 1. The equilibrium 2 NO(8) + Cl2te) = 2 NOCI(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm and 0.28 atm for NO, Cl2 and NOCI, respectively. Calculate the Kp for this reaction at 500 K. 2. Phospho

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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4. IBr decomposes according to the reaction at 150 C: 2 IBr (g) = I2 (g) + Br2 (g) If IBr is placed in a container at an initial pressure of 5.0 atm, what will be its %3D equilibrium pressure at 150°C? Kp = 8.3 x 10-3
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
3. A reaction vessel is filled with SO, at a partial pressure of 0.10 atm together with O, and SO,, both of which are at a partial pressure of 0.20 atm. The equilibrium constant, Kp, for the oxidation of SO, is equal to 0.15 at 900°K. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 2SO,(g) + .(3)0 0,(g) = 2S0,(g) Кр Kp = 0.15 at 900°K
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F5 -5 At 35°C, K = 1.8 x 10 for the reaction 2 NOCI(g) 2 NO(g) + Cl₂ (g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.4 moles of pure NOCI in a 2.0-L flask. [NOCI] = M [NO] = [Cl₂] = = M b. 1.0 mole of NOC1 and 1.0 mole of NO in a 1.0-L flask [NOCI] = [NO] = M [Cl₂] = M c. 2.0 mole of NOCI and 1.0 mole of Cl₂ in a 1.0-L flask [NOCI] = = M [NO] = [Cl₂] Submit Answer 6 Show Hint H F6 & 7 = Retry Entire Group KI F7 * 8 DII FB Topics] K M M 9 M ( M 9 more group attempts remaining D F9 [References] O ) O F10 P J F11 Previous Next Save and Exit F12 delete
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.79 at a certain temperature. If a reaction mixture initially contains 0.050 M H2S and 0.050 M SO2, what will the equilibrium concentration of H2O be? 2 H2S(g) + SO2(g)=3 S(s) + 2 H20(g) 1 NEXT > Based on the given values, set up ICE table in order to determine the unknown. 2 H2S(g) SO2(g) 3 S(s) 2 H20(g) + + Initial (M) |Change | (M) Equilibrium | (M) 5 RESET 0.050 +x +2x +3x -x -2x -3x 0.050 + x 0.050 + 2x 0.050 + 3x 0.050 - x 0.050 - 2x 0.050 -3x 0.025 + x 0.025 + 2x 0.025 + 3x 0.025 - x 0.025 - 2x 0.025 -3x
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In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC. In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first. This mixture is also heated to 350 oC. After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?
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