A chemist is studying the following reaction that has an equilibrium constant of 6.5 x 10² 1/M 2NO(g) + 2H₂ (8) N₂ (g) + 2H₂O(g) She measures the concentrations of all of the chemicals in her beaker. . [NO] -0.089 M • [H₂] -0.035 M . [N₂] -0.008 M . [H₂0] -0.098 M Based on the concentrations she measured, is this reaction currently at equilibrium? If not, which way must the reaction shift to attain equilibrium? O Yes, it is at equilibrium O No, it is not at equilibrium. It needs to shift toward the products O No, it is not at equilibrium. It needs to shift toward the reactants O There is not enough information to solve this problem.

A chemist is studying the following reaction that has an equilibrium constant of 6.5 x 10² 1/M 2NO(g) + 2H₂ (8) N₂ (g) + 2H₂O(g) She measures the concentrations of all of the chemicals in her beaker. . [NO] -0.089 M • [H₂] -0.035 M . [N₂] -0.008 M . [H₂0] -0.098 M Based on the concentrations she measured, is this reaction currently at equilibrium? If not, which way must the reaction shift to attain equilibrium? O Yes, it is at equilibrium O No, it is not at equilibrium. It needs to shift toward the products O No, it is not at equilibrium. It needs to shift toward the reactants O There is not enough information to solve this problem.

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

Consider the reaction. A(aq) = 3 B(aq) K. = 8.37 x 10-6 at 500 K If a 4.30 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = M * TOOLS x10
9. Consider the reaction: 2 A (g) + 3 B (g) = 2 C (g) + 4 E (g). The reaction is initiated with 0.60 M in A, 0.45 M in B and 0.50 M in E (Note 0 M in C). At equilibrium, the value of [B] = 0.15 M. What is the equilibrium value of [E]? a) 0.95 M b) 0.90 M c) 0.80 M d) 0.60 M e) 0.50 M f) 0.40 M g) none of the above 0 4 15 Determine the acid ionization constant
QUESTION 4 For the reaction at 20. °C, NH3(aq) +H(aq) NH4 (aq) The equilibrium constant is calculated to be K - 4.5 x 108 If a base (NaOH) was added to the mixture, the hydroxide ion, OH", would react with the H* to form water. This would decrease the concentration of H* in the solution. How would this affect the concentration of NH4 *? OaThe concentration of NH4* would increase. Ob. The concentration of NH4 would decrease. OCThe concentration of NH4* would remain unchanged.
The ionization product of water, k_WkW, is usually approximated to be 1.0 x 10-14. The chemical equation for the ionization product of water is: 2H2O <==><==> H3O+ + OH- Thinking about the definition of equilibrium constants and then specifically k_WkW, explain why k_WkW is written without units
Please, help me with this question. Consider the reaction. A(aq)↽−−⇀3B(aq) ?c=8.50×10−6 at 500 K If a 2.50 M sample of A is heated to 500 k, what is the concentration of B at equilibrium?
Consider the reaction. A(aq) 2 3 B(aq) K. = 7.25 × 10 6 at 500 K If a 5.10 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = TOOLS x10 privacy policy terms of use contact us help сareers eq_science_c..doc fle 三 * 66| 99+ DELL
Which statements are always correct for a reaction at equilibrium? The forward and reverse reactions both continue. The concentrations of reactants and products are equal. The rates of the forward and reverse reactions are equal. I. II. |||. OII and III only I and III only I, II, and III I and II only
Consider the equilibrium reaction. H₂(g) + 1₂(9) ⇒ 2 HI(g) In this case, 1.000 M H₂ reacts with 2.000 M of 1₂ at a temperature of 430.ºC. The value of K = 68. Determine the equilibrium concentrations of H₂, I₂, and HI. C M [H₂] [1₂] M [HI] M
At a certain temperature, the equilibrium constant for the chemical reaction shown is 3.86×10−33.86×10−3. At equilibrium, the concentration of AB is 2.6252.625 M, the concentration of BC is 2.8252.825 M, and the concentration of AC is 0.1300.130 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq)
13) The reaction of bromine gas with chlorine gas, shown below, has a Kc of 1.45 at 230 oC. If a closed vessel was charged with 0.500 M BrCl, what would be the equilibrium concentration (M) of BrCl(g)? Br2(g) + Cl2(g) ó 2 BrCl a) 0.344b) 0.156c) 0.226d) 0.188e) 0.425f) 0.0122
One more: H2 + I2 <----> 2HI. If K=50, what is the equilibrium concentration of HI if the initial concentration of HI is 0.10?
Hi, Write an equilibrium expression for chemical equation involving one or moresolid or liquid reactants or products, thanks. CO32-(aq)+ H2O(l) <-----> HCO3-(aq) + OH-(aq)