The statements in the tables below are about two different chemical equilibria. The symbols have their usual meaning, for example AG° stands for the standare Gibbs free energy of reaction and K stands for the equilibrium constant. In each table, there is one statement that is false because it contradicts the other three statements. When you find a false statement, check the box next to it. statement false? statement false? AG°<0 AG°>0 K<1 K>1 AH°>TAS° In K<0 In K>0 AH°

The statements in the tables below are about two different chemical equilibria. The symbols have their usual meaning, for example AG° stands for the standare Gibbs free energy of reaction and K stands for the equilibrium constant. In each table, there is one statement that is false because it contradicts the other three statements. When you find a false statement, check the box next to it. statement false? statement false? AG°<0 AG°>0 K<1 K>1 AH°>TAS° In K<0 In K>0 AH°

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 reactions and their respective equilibrium constants: NO(g) + ½Br₂(g) = NOBr(g); K = 5.3 2NO(g) = N₂(g) + O₂(g); K = 2.1 × 10³⁰ Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: N₂(g) + O2(g) + Br₂(g) = 2NOBr(g) Express your answer using two significant figures.
Consider the following chemical equilibrium: 4 NH, (g) +3 0, (g)=2N, (g) +6 H,Oo (g) Now write an equation below that shows how to calculate K, from K, for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K_ = I
produces N20 and oxygen. Calculate the value of the equilibrium constant K. for the reaction 2 N,O4(g) –2 N,0(g) + 3 O2(g) from the following information: N2(g) + ¿O2(g) =N‚O(g) K¸ = 2.7 × 10-18 N,O4(g) =2 NO;(g) K. = 4.6 × 10-3 N2(g) + 2 O2(g) =2 NO2(g) K. = 1.7× 10-17
Phosgene is a chemical warfare agent first used on soldiers in World War I. It is synthesized according to the following gas-phase equilibrium reaction: CO(g) + Cl, (g) = COCI,(g) Write the equilibrium expression K, for this reaction below. K. = If K. = 0.281 for this reaction, would the product or the reactant be favored at equilibrium? The reactants would be favored. Neither the product nor the reactants would be favored. The product would be favored.
At 100 0 C the equilibrium constant for the reaction COCl 2 (g) = CO (g) + Cl 2 (g) has the value of Kc = 2. 19 x 10 – 10 . Predict the direction in which the system will move to reach equilibrium from the following given concentrations: A) [ COCl 2 (g)] = 5. 00x 10 – 2 M ; [ CO (g) ] = 3. 31 x 10 – 6 M ; [ Cl 2 (g) ] = 3. 31 x 10 – 6 M B) [ COCl 2 (g)] = 1. 45 M ; [ CO (g)] = 1. 56 x 10 – 6 M ; [ Cl 2(g)] = 1. 56 x 10 – 6 M
Consider the following chemical equilibrium: C(s) + 2 H₂ (g) ⇒ CH₂(g) Now write an equation below that shows how to calculate K from K for this reaction at an absolute temperature T. You can assume I is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K -0 X 00
The statements in the tables below are about two different chemical equilibria. The symbols have their usual meaning, for example AGO stands for the standard Gibbs free energy of reaction and K stands for the equilibrium constant. In each table, there may be one statement that is false because it contradicts the other three statements. If you find a false statement, check the box next to it. Otherwise, check the "no false statements" box under the table. statement In K0 AH
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The equilibrium constant, Kc, is given for one of the reactions below. What is the value of the missing equilibrium constant, Ke? Cl₂(g) + H₂O(g) = 2 HCl(g) + O₂(g) K = 7.52 x 10-² 4 HCI(g) + O₂(g) = 2 Cl₂(g) + 2 H₂O(g) K = ? OK=177 K = 0.150 OK-5.66 x 10-3 OK 13.3 3 pts ) K = 3.65
Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N₂(g) + O₂(g) 2NO(g) Ke=4.3 × 10-25 2NO(g) + O₂(g) = 2NO₂(g) K=6.4 × 10⁹ Determine the value of the equilibrium constant for the following equation at the same temperature: N₂(g) +20₂(g) = 2NO₂(g) Ke= 10 (Enter your answer in scientific notation.)
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