Match the Term with the definition 1. Equilibrium position 2. Chemical equilibrium 3. Reaction quotient 4. Law of mass action 5. Equilibrium constant C a. used to determine if a reaction has reached equilibrium b. depends on the initial concentrations of the substances in a reaction c. states that every reaction proceeds to an equilibrium state with a specific Keq d. the point at which the reaction appears to "stop" e. the ratio of product concentration to reactant concentration at equilibrium 6. For the reaction N2 (g) + O2(g) 2 NO(g) that is run at 25 °C, Kc = 1.2 × 10-30. Use this information to calculate the equilibrium co for the reaction 2 NO(g) N2 (g) + O2(g) a. 8.3 x 1029 b. 1.2 x 10-30 C. 1.7 x 1030 d. 1.1 x 10-15 e. 6.0 × 10-31 7. Write the equilibrium expression for the formation of nitrosyl bromide. a. [NO] 2 [Br]/[NOBr] 2 b. [NOBr]2/[NO] 2 c. [NOBr] 2/[NO] 2 [Br2] d. [NO] 2[Br2] / [NOBr] 2 e. [NOBr] 2/[NO]² 2NO(g) + Br2 (g) 2NOBr(g)

Match the Term with the definition 1. Equilibrium position 2. Chemical equilibrium 3. Reaction quotient 4. Law of mass action 5. Equilibrium constant C a. used to determine if a reaction has reached equilibrium b. depends on the initial concentrations of the substances in a reaction c. states that every reaction proceeds to an equilibrium state with a specific Keq d. the point at which the reaction appears to "stop" e. the ratio of product concentration to reactant concentration at equilibrium 6. For the reaction N2 (g) + O2(g) 2 NO(g) that is run at 25 °C, Kc = 1.2 × 10-30. Use this information to calculate the equilibrium co for the reaction 2 NO(g) N2 (g) + O2(g) a. 8.3 x 1029 b. 1.2 x 10-30 C. 1.7 x 1030 d. 1.1 x 10-15 e. 6.0 × 10-31 7. Write the equilibrium expression for the formation of nitrosyl bromide. a. [NO] 2 [Br]/[NOBr] 2 b. [NOBr]2/[NO] 2 c. [NOBr] 2/[NO] 2 [Br2] d. [NO] 2[Br2] / [NOBr] 2 e. [NOBr] 2/[NO]² 2NO(g) + Br2 (g) 2NOBr(g)

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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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.
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Question 29 of 30 Consider the reaction of N2O and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 NO(g) +3 O₂(g) 4 NO2(g) 1 2 NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O2 and 0.200 mol N2O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. 2N₂O(g) + 302(g) == 4NO2(g) Initial (M) 0.200 -0.0100 0.190 Change (M) 0.0560 -0.0150 0.0410 Equilibrium (M) 0 0.0200 0.0200 RESET 0 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190
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13. H.(g)+F(g) = 2HF(g) At this temperature, 0.481 Kc =9.41 x 10³ mol H₂ and 0.481 mol F₂ were placed in a 0.750 L container to react. What concentration of HF is present at equilibrium? a. 0.588 M b. 0.600 M c. 1.18 M d. 1.20 M #431 10 e. 1.79 M السلام امن mla