Answered: Calculate the composition of the…

Calculate the composition of the gaseous mixture obtained when 4.95 mol of carbon dioxide is exposed to hot carbon at 840°C in a 3.35 L vessel. The equilibrium constant Kc at 840°C is 2.51

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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A student ran the following reaction in the laboratory at 1080 K: 2SO3(g) 2S02(g) + O₂(g) When he introduced SO3(g) at a pressure of 0.886 atm Into a 1.00 L evacuated container, he found the equilibrium partial pressure of SO3(g) to be 0.340 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer 44 $ T R F V/ % 5 Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support F5 G ^ 6 MacBook Air Y H & 7 RN U * 0 J ► 11 F8 M ( 9 ►► K F9 O 1 F11 + { Save and Exit = F12 11
The chemical equation given below indicates a hypothetical reaction. A(a9) + 3 B(ag) = 2 C(ag) + D(ag) A mixture of 4.00 mol A and 5.00 mol B are placed in a container and allowed to come to equilibrium. Find the amounts of A, B, and C if the mixture contains 0.75 mol D at equilibrium. Complete the ICE table and consider that there are no C and D at the beginning.
At a certain temperature, the equilibrium constant K for the following reaction is 734.: NO3(g) + NO(g) 2 NO₂(g) Use this information to complete the following table. ?
part b
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
A 13.4 L reaction vessel at 483°C contained 0.892 mol , H2, 0.620 mol I2, and 5.41 mol . HI. Assuming that the substances are at equilibrium, find the value of Kc at 483°C for the reaction of hydrogen and iodine to give hydrogen iodide. The equation is H2(g)+I2(g)->2HI(g) Kc=_________
H2. Please give typed answer
NA van wwwwwwww 1. For the reaction, 2 NO (g) + 2 H₂ (g) = following equilibrium concentrations: [NO]= 8.1 x 10-³ M [N2] = 0.053 M N₂ (g) + 2 H₂O (g), calculate Keq given the [H₂] = 4.1 x 10-5 M [H₂O]= 2.9 x 10-³ M 2. Given the reaction, UO2 (g) + 4 HF (g) = UF4 (g) + 2 H₂O (g), predict the effect each of the following will have on the equilibrium of the reaction (shift to the reactant side, the product side, or no shift). a. Uranium dioxide (UO2) is added. c. Water vapor is removed. b. Hydrogen fluoride (HF) reacts with the walls of the reaction vessel. - 3. At a certain temperature, Keq = 150 for the reaction being studied in today's lab. Use Equation (3) to calculate the concentrations of Fe³+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 105 M. Assume the equilibrium concentrations of Fe³+ and SCN are equal.
▸ 69 20 E Consider the following system at equilibrium at 723 K: N₂(g) + 3H₂(g) 2NH3(g) + 26.6 kcal Indicate whether each individual change would favor the production of NH3(g). Evaluate each change separately, assuming that all other conditions remain constant. D Decreasing the temperature. Decreasing the pressure. Increasing the volume. Removing NH3. Removing H₂. C Submit Answer $ 4 R F % 5 V Retry Entire ♫ FS T G [References] the References to access important values if needed for this question. A 6 v yes no B MacBook Air F6 3 more group attempts remaining Y H & 7 B F7 U N * 8 00 D--ll FB J J ( T 1 M 9 K DD FO O O L ge A F10 P command Previous Email Instructor 4 i A AN = Next> Save and Exit ( { ? 912 option delete retu