Consider the following reaction:H₂ (g) + 12 (g) = 2 HI(g)Complete the following table. Assume that allconcentrations are equilibrium concentrations in M.T (°C) [H₂]HI K.]0.03550.922253404454.90x10-2M0.03884.50x10-2 0.384MM4.68x10-2M-90.650.2Find [H₂] at 340 °C.Express your answer using two significant figures.195| ΑΣΦΑ[H₂] =Submit Previous Answers Request Answer?M

Answer: Equilibrium constant is the ratio of molar concentrations of products and molar…

Consider the following reaction: H₂ (g) + 12 (g) 2 HI(g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T (°C) [H₂] 25 340 445 0.0355 [HI K.) 0.0388 0.922 4.50x10-2 0.384 M M 4.90x102 4.68x10-2 M M 90.6 50.2 Find (H₂) at 340 °C. Express your answer using two significant figures. [H₂])- 195| ΑΣΦΑ Submit Previous Answers Request Answer ? M

Consider the following reaction: H₂ (g) + 12 (g) 2 HI(g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T (°C) [H₂] 25 340 445 0.0355 [HI K.) 0.0388 0.922 4.50x10-2 0.384 M M 4.90x102 4.68x10-2 M M 90.6 50.2 Find (H₂) at 340 °C. Express your answer using two significant figures. [H₂])- 195| ΑΣΦΑ Submit Previous Answers Request Answer ? M

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

Calculate the equilibrium concentrations for all reactants and products if initial concentrations of CH4 is 0.400 M, H2S is 0.800 M, CS2 is 0.400 M, H2 is 0.800 M are mixed and allowed to establish equilibrium. The Kc for the reaction is 0.0360 and the equilibrium concentration of CH4is 0.556 M. CH4(g) + 2H2S(g) ↔ CS2(g) + 4H2(g) Group of answer choices [CH4] = 0.556 M, [H2S] = 0.488 M, [CS2] = 0.556 M, [H2] = 1.42 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.244 M, [H2] = 0.176 M. [CH4] = 0.556 M, [H2S] = 0.244 M, [CS2] = 0.956 M, [H2] = 1.36 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.556 M, [H2] = 1.42 M.
NAME: COC12(g) has a 8. At 100.0°C, the equilibrium constant for the reaction: COg) + Cl2(g) value of 4.6 x 10°, If 0.40 mol of COC12 is placed into a 10.0 L flask at 100.0°C, what will be the equilibrium concentration of all species? (A simplifying approximation that will make the solution of the resulting equation easier is to note that X is much less than 0.040 mol/L. This means that 0.040-x is approximately 0.040.)
Consider the following equilibrium: CO(g) + 3 H2(g)-CH4(g) + H2Og). If K, = 1.61 x 10-5 at 1400.0 K, calculate K. O 0.212 O 1.40 x 107 O 1.85 x 103 O 541 O 1.22 x 10-9 « Previous Next
20
consider the reaction h2(g) + f2(g) 2hf(g) with the equilibrium constant k = 100. at some temperature. a) how many moles of h2(g) must be mixed with 1.00 moles of f2(g) in a 1.00 I high-pressure flask to produce 1.70 moles of hf(g) once the flask reaches equilibrium?
N2(g) and O2(g) can exist in equilibrium with NO(g), as shown below. The equilibrium constant at 25.0°C is 4.8 x 10-31. If initially there are 1.35 mol of nitrogen and 0.60 mol of oxygen in a 2.00 L vessel, find the equilibrium concentrations of each species. N2(g) + O2(g) → 2NO(g)
Consider the reaction A + B C+D, which has an equilibrium constant, K, equal to 3.4 x 102. If one begins a reaction by placing 0.600 moles of A in a 1.0 L container as well as 0.150 moles of 1. B, what will be the equilibrium concentrations of A, B, C, and D? Write your answers in the spaces provided below. a. [А] b. [B]= [C]= С. d. [D]= Once the reaction in problem 1 reaches equilibrium, some additional B is injected into the flask 2. from an outside source. LeChatelier's principle says the reaction will (circle one): be unchanged shift to the right shift to the left Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L of 3. water, what will be the equilibrium concentrations of the species below: a. [Pyridine] = b. [Pyridine-H] (the pyridinium ion) [ОН-] 3 С. What is the pH of the solution in problem 4 (above)? .
Consider the following reaction at 400°C and its equilibrium constant: 2 HI(g) - 12(g) + H2(g) Kc = 0.0156 A reaction mixture contains 0.420M I2, 0.420 M H, and 3.36 M HI. Which of the following statements is TRUE? The reaction will shift in the direction of the products. The reaction quotient will decrease. The equilibrium constant will increase. OThe reaction will shift in the direction of the reactants. The system is at equilibrium.
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.
What is the expression of equilibrium constant K for overall reaction?
6. Write the equilibrium constant expression for the following reactions. a. CHa (8) + 20; (B) → CO; (B) + 2H;0 (g) b. 4 NH3 (g) + 302 (g) → 2N2 (g) + 6H;0 (g) c. C (s) + 2H2 (g) CH4 (g)