Concept explainers
Interpretation:
From the given options, the one which is not the characteristic of a chemical system in an equilibrium state has to be chosen.
Concept Introduction:
It is a point at which the rate of the forward reaction equals to the
Reversible Reaction:
Reaction in which, the product formed get reacts and give back the reactants. It will attain equilibrium where the concentrations of product and reactant will not change thereafter
Example:
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Chapter 9 Solutions
EBK GENERAL, ORGANIC, AND BIOLOGICAL CH
- Which of the following is the correct equilibrium constant expression for the reaction 3C(g)A(g)+2B(g) a. [A] [2B]/[3C] b. [3C]/[A] [2B] c. [A] [B]/[C] d. no correct responsearrow_forwardThe reaction C,H2 (g) + 2F2 (9) C,H,F(g) is exothermic in the forward direction. Will an increase in temperature shift the position of the equilibrium toward the reactants or products? O It will shift the position of the equilibrium toward the products. O It will shift the position of the equilibrium toward the reactants. O There is no change on the position of equilibrium. Submit Answer Try Another Version 1 item attempt remainingarrow_forwardBelowarrow_forward
- C2H4 (colorless) + I2 (violet) → C2H4I2 (colorless) + heat An equilibrium is established in the reaction above. What change would ber observed in the appearance of the quilibrium mixture if a catalyst was added? a. no change would be seen b. the violet color of the mixture would become lighter c. the violet color of the mixture would become darker d. no correct responsearrow_forwardSaved Enabled: Exam 2 i Which statement is correct? Multiple Choice None of the answers is correct. if Q K then reactants must be converted to products. if Qarrow_forwardWe use an ICE table to solve for equilibrium concentrations when given initial concentrations and the equilibrium constant, K. For each case below, determine the best approach to solve for x using the value of K and the expression of K with x. "x" represent the smallest positive change. Solving approach Case 1 Case 2 Case 3 Case 4 K expression 2² (0.5-2)2 K = 0,5-z K= K K= 0.5-a 0.5- K value 0.64 0.80 0.86 1.3 x 10-7 ✔ [ Select] direct solving with quadratic equation assuming x is small taking square root direct solving without quadratic equation [Select] [Select]arrow_forwardProblem 4 Review I Cc For the reaction 2CO (g) +02(g) = 2CO 2 (g ) , the equilibrium concentrations at a certain temperature are [CO2] = 0.10 mol/L, [02] = 1.7x102 mol/L, [CO] - 2.4x102 mol/L. Part B What is the value of Kat this temperature? Express your answer using two significant figures. ΑΣφ ? K = 25 Previous Answers Request Answer Submit x Incorrect; Try Again; 5 attempts remaining Part C Are reactants or products favored? P Pearson 2019 Pearson Education Inc. All rights reserved. | Terms of UseI Privacy Policy Permissions Contact Us Copyrightarrow_forward17.42 Even at high T, the formation of NO is not favored: N(g) + 0(g) 2NO(g) K. = 4.10X10 4 at 2000° Carrow_forwardAt a particular temperature, K = 3.1 for the reaction SO2 (9) + NO2(9) SO3(9) + NO(9) If all four gases had initial concentrations of 0.800 M, calculate the equilibrium concentrations of the gases. [SO2] = м [NO2] = M [SO3] = M %3! [NO] = %3! Submit Answer Try Another Version 3 item attempts remainingarrow_forwardConsider the following hypothetical reactions. The equilibrium constants K given for each reaction are defined in terms of a concentration unit of molecules per liter. A(g)B(g)K=2X(g)2Y(g)K=62C(g)D(g)K=1 Assume that the reactions have reached equilibrium. Match each of these reactions with one of the containers I to IV (each of which has a volume of 1 L). Identify the color of each molecule (for example, is A red or blue?).arrow_forwardExercise 17.5 For the exothermic reaction 2SO2(g)+O2(g)2SO3(g)predict the equilibrium shift caused by each of the following changes. a. SO2is added. b. SO3is removed. c. The volume is decreased. d. The temperature is decreased.arrow_forwardPls answer correct and explanation fastarrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
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