Consider the following reaction where Kc = 7.00 x 10-5 at 673 K. NH4I(s) NH3(g) + HI(g) A reaction mixture was found to contain 0.0532 moles of NH4I(s), 0.00571 moles of NH3(g), and 0.00837 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals The reaction O must run in the forward direction to reach equilibrium. Omust run in the reverse direction to reach equilibrium. Ois at equilibrium.

Consider the following reaction where Kc = 7.00 x 10-5 at 673 K. NH4I(s) NH3(g) + HI(g) A reaction mixture was found to contain 0.0532 moles of NH4I(s), 0.00571 moles of NH3(g), and 0.00837 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals The reaction O must run in the forward direction to reach equilibrium. Omust run in the reverse direction to reach equilibrium. Ois at equilibrium.

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...

See similar textbooks

Similar questions

For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.220 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.
The equilibrium constant, K, for the following reaction is 2.90×10-2 at 1.15×10³K. 2S03(g) 2S02(g) + 02(g) If an equilibrium mixture of the three gases in a 14.5 L container at 1.15×10³K contains 0.367 mol of SO3(g) and 0.356 mol of SO2, the equilibrium concentration of O, is M.
CO2 and H, are allowed to react until an equilibrium is established as follows: CO2 (g) + H, (g)H,0 (g) + CO (g) What will be the effect on the equilibriumn of removing CO from the equilibrium mixture?
Enter your answer in the provided box. For the reaction H₂(g) + CO₂(g) H₂O(g) + CO(g) at 700°C, K, 0.534. Calculate the number of moles of H₂ that are present at equilibrium if a mixture of 0.700 mole of CO and 0.700 mole of H₂O is heated to 700°C in a 50.0-L container. mol
Consider the following reaction where K, = 55.6 at 698 K. H2(g) + I2(g) =2HI(g) A reaction mixture was found to contain 2.94×102 moles of H2(g), 4.25×102 moles of I2(g) and 0.301 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCI3(g) + Cl₂(g) PCI5(g) Calculate the equilibrium concentrations of reactant and products when 0.587 moles of PCI3 and 0.587 moles of Cl₂ are introduced into a 1.00 L vessel at 500 K. [PCI3] = [Cl₂] [PCI 5] = = M M M
Gaseous NO is placed in a closed container at 477 oC, where it partially decomposes to NO2 and N2O: 3 NO(g) 1 NO2(g) + 1 N2O(g) At equilibrium it is found that p(NO) = 0.009840 atm, p(NO2) = 0.008270 atm, and p(N2O) = 0.008870 atm. What is the value of KP at this temperature?KP =
Hydrogen iodide decomposes according to the reaction 2HI(g) = H₂(g) + 1₂ (g) A sealed 1.50-L container initially holds 0.00623 mol of H₂, 0.00414 mol of 1₂, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H₂(g) is 0.00524 M. What are the equilibrium concentrations of HI (g) and I₂ (g)? Round each of your answers to 3 significant figures. Part 1 of 2 [HI] = M Part 2 of 2 [¹2]eq = M x10 x10 X x Ś S
The equilibrium constant, K. , for the following reaction is 1.80x10 at 298 K. NH,HS(s) NH3(g)+ H,S(g) If an equilibrium mixture of the three compounds in a 6.85 L container at 298 K contains 1.56 mol of NH HS(s) and 0.468 mol of NH3, the number of moles of H,S present is moles.
Consider the equilibrium between SbCl5, SbCl3 and Cl₂. SbCl5(g) SbCl3(g) + Cl₂(g) K = 2.46x10-² at 530 K The reaction is allowed to reach equilibrium in a 7.30-L flask. At equilibrium, [SbCl5] = 0.430 M, [SbCl3] = 0.103 M and [Cl₂] = 0.103 M. (a) The equilibrium mixture is transferred to a 14.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.6-L flask. [SbCl5] = [SbCl3] = [Cl₂] |||| ΣΣΣ
Consider the following reaction where Kc = 55.6 at 698 K.H2(g) + I2(g) 2HI(g)A reaction mixture was found to contain 4.52×10-2 moles of H2(g), 4.50×10-2 moles of I2(g) and 0.298 moles of HI(g), in a 1.00 liter container.Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals .The reactionfill in the blank 2A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium. Submit Answer
Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 8.62×10-3 moles of COCl2, 0.353 moles of CO, and 0.282 moles of Cl2 are at equilibrium in a 12.5 L container at 757 K, the value of the equilibrium constant, Kp, is .