2. Consider the following reaction: COCl2(g) <--> CO(g) + Cl₂(g) A reaction mixture initially contains 1.6 M COCI2. Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. A) 3.7 × 10-2 M B) 1.5 × 10-3 M C) 4.2 × 10-4 M D) 2.1 × 10-2 M -3

2. Consider the following reaction: COCl2(g) <--> CO(g) + Cl₂(g) A reaction mixture initially contains 1.6 M COCI2. Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. A) 3.7 × 10-2 M B) 1.5 × 10-3 M C) 4.2 × 10-4 M D) 2.1 × 10-2 M -3

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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At a certain temperature, the reaction PCl5(g) <====> PCl3(g) + Cl2(g) has an equilibrium constant Kc=5.8x10^-2 a) calculate Kc for the synthesis of 2 moles of PCl5(g) at the same temperature
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
Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N2O4(g) 2 NO2(g) Three experiments were run starting with different initial amounts of N2O4(g) ([N2O4]0 in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter).For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO2 and N2O4 at equilibrium.Be sure to round to the correct number of significant figures. Exp [N2O4]0 [NO2] [N2O4] [NO2] / [N2O4] 2 [NO2] / [N2O4] [NO2]2 / [N2O4] 1 3.7 2.92 2.2 2 2.8 2.49 1.6 3 2.6 2.33 1.4 Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N2O4. 2. The…
Consider the equilibrium system described by the chemical reaction below. When 1.50 mol of CO₂ and an 10.0 mol solid carbon are heated in a 20.0 L container at 1100 K, the equilibrium concentration of CO is 0.0700 M. Determine the concentrations of all species at equilibrium and then calculate the value of Kc for this reaction. C(s) + CO₂(g) 2 CO(g) NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) 0 1.50 1 C(s) 10.0 + 20.0 CO₂(g) 2 0.500 2 CO(g) 0.150 RESET 0.0750 +
2
Consider the following chemical equilibrium: N₂ (g) + 3H₂(g) 2NH3(g) с Now write an equation below that shows how to calculate K from K for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K₁ = 0 P 00 X 5 010
3. Consider the following equilibrium reaction: H2(g) + F2(g) 2HF Keq = 2.4 x 10-³ (at a given temperature) Calculate the concentration of HF if [H2] = 0.0031 M and F2 = 0.0054 M.
6. On analysis, an equilibrium mixture for the reaction: 2 H,S( ) was found to contain 1.0 mol H,S, 20.0 mol H, and 0.80 molS, in a 4.0 L vessel. Calculate the equilibrium constant (Kc) for this reaction. 2 H,(g) + S,(g) 2' 51 80 O 13 29 3
The equilibrium constant, K, for the following reaction is 1.0 x 10 -5 at 1500 K. N2(g) + O2(g) <---> 2 NO(g) If 0.750 M N2 and 0.750 M O2 are allowed to reach equilibrium at 1500 K, what is the concentration of NO? a. 2.4 x 10-3M b. 6.7 x 10-4M c. 5.5 x 10-3M d. 2.7 x 10-3M e. 1.2 x 10-3M
2. Temperature can have a significant effect on the value of the equilibrium constant. For example, the dissociation of Ca(OH), has a Ksp of 6.5 x 10 * at 20 °C and a Ksp of 5.5 x 10 * at 25 °C. Is the dissociation of Ca(OH), an exothermic or endothermic process? Fully explain your answer.
Question 13 of 50 Consider the equilibrium system described by the chemical reaction below. When 1.50 mol of CO, and an 10.0 mol solid carbon are heated in a 20.0 L container at 1100 K, the equilibrium concentration of CO is 0.0700 M. Determine the concentrations of all species at equilibrium and then calculate the value of Kc for 2 this reaction. C(s) + CO,(g) =2 CO(g) 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C(s) CO,(9) 2 СО(g) + Initial (M) Change (M) Equilibrium (M) 5 RESET 1.50 10.0 20.0 0.500 0.150 0.0750 0.0700 -0.0700 0.140 -0.140 0.0350 -0.0350 0.110 0.0400 0.0050 1L