QUESTION 6 Chemical Equilibrium Which statement is true about a chemical reaction which is at equilibrium? Equilibria.pdf O A. The reverse reaction has reached completion. OB. The temperature of the forward reaction is equal to the rate of the reverse reaction. O C. The mass of the products is equal to the mass of the reactants. O D. The forward reaction rate is equal to the reverse reaction rate. O E. The forward reaction has reached completion.

QUESTION 6 Chemical Equilibrium Which statement is true about a chemical reaction which is at equilibrium? Equilibria.pdf O A. The reverse reaction has reached completion. OB. The temperature of the forward reaction is equal to the rate of the reverse reaction. O C. The mass of the products is equal to the mass of the reactants. O D. The forward reaction rate is equal to the reverse reaction rate. O E. The forward reaction has reached completion.

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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Consider the following equilibrium: N204(g) 2 2NO2(g) A 1.00 L container is initially filled with 0.200 mole N204. At equilibrium, 0.160 mole NO2 are present. What is the equilibrium concentration of N204? a. 0.120 mole/L b. 0.080 mole/L c. 0.040 mole/L d. 0.160 mole/L
Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed? a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases
Define equilibrium in terms of a)reaction rates -Forward reaction rate = reverse reaction rate b)changes in observable properties -There are no observable changes c)energy and energy changes -Energy has become stable (no longer giving off or taking in heat)
Given the Equilibrium Equation: CO (g) + Cl2 (g) <--> COCl2 (g) and ΔH = -25.9 kcal/mole Which option would make the equilibrium shift towards the products? Pick all that apply. (There may be multiple answers that are correct) a. adding more phosgene b. adding more carbon monoxide c. increasing the temperature d. decreasing the reaction container volume e. decreasing the temperature
4 NH3(g) +5 O2(g) = 4 NO(g) + 6 H,0(g) AH =-904.4 kJ Consider the equilibrium system represented in the reaction above. Will the concentration of NO increase, decrease, or remain the same when the following experimental changes are made: a. NH, is added d. The volume of the container is reduced b. [H,O] is increased e. A catalyst is added c. O, is removed f. The temperature is increased
If we represent the equilibrium as: 2 NO2(g) = N204(g) We can conclude that: |1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
QUESTION 4 Adding a catalyst to an equilibrium system will: produce more products at equilibrium. produce more reactants at equilibrium. not change the amount of reactants or products at equilibrium.
Chemical or physical processes that can proceed in both the forward and reverse directions are called reversible processes redox processes O combustion processes equilibrium processes Next • Previous
Given each equilibrium constant, state whether the reactants are favored, the products are favored, or both the reactants and products are present at equilibrium. a. 5.0 × 10 −4 b. 4.4 × 10 5 c. 350 d. 0.35
6. Consider the reaction: N2 (g) + 3 H2 (g) = 2 NH3 (g) Complete the table below, assuming all concentrations are equilibrium concentrations in. molarity. TK IN2] [H2] ENH3] Kc 500 0.115 0.105 0.439 575 0.110 0.128 9.6
For questions 9-13. Consider the reaction 2NOCI(g) = 2NO(g) + C12(g). If this reaction is at equilibrium, what happens when the following changes occur? 9. NOCI(g) is added O shift to right shift to left no reaction O both shifts to right and left
I. 2NOCl (g)< < > 2NO(g) + Cl2(g) K= 1.6X 10-5 II. 2NO (g) < > N2(g) + O2(g) K= 1.0 X 1031 Which of the following will you choose to generate the most amount of NO? (Think which of the reactions will favor the formation of NO.)a.Forward reaction of IIb.Forward reaction of Ic.Reverse reaction of Id.Reverse reaction of II