SO₂ reacts with Cl₂ to form SO₂Cl₂. The equilibrium constant, Kp, for this reaction is 0.417 at 373 K. 4 SO₂(g) + Cl₂(g) SO₂Cl₂(g) The standard enthalpy change for this reaction (AH°) is -67.2 kJ/mol. (a) Predict the effect on the production of SO₂Cl₂ when the temperature of the equilibrium system is increased. (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 449 K. Kat 449 K =

SO₂ reacts with Cl₂ to form SO₂Cl₂. The equilibrium constant, Kp, for this reaction is 0.417 at 373 K. 4 SO₂(g) + Cl₂(g) SO₂Cl₂(g) The standard enthalpy change for this reaction (AH°) is -67.2 kJ/mol. (a) Predict the effect on the production of SO₂Cl₂ when the temperature of the equilibrium system is increased. (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 449 K. Kat 449 K =

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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A student dissolves 14.9 g of potassium hydroxide (KOH)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 23.0 °C to 33.0 °C over the course of 5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: KOH(s) K+ (aq) + OH(aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ. per mole of KOH. rxn exothermic…
Consider the general reaction 2A(g) + B(s) = C(g) +3D(g) AH = +115 kJ which has already come to equilibrium The position of the equilibrium was shifted by adding additional B(s) to the system. Choose the correct effect on equilibrium (it will shift to the right, will shift to the left, or it will not be affected). O It will shift to the right. O It will shift to the left. O It will not be affected Consider the general reaction 2A(9) + B(s) C(g) + 3D(g) AH = +115 kJ which has already come to equilibrium. The position of the equilibrium was shifted by removing C(g) from the system as it forms. Choose the correct effect on equilibrium (it will shift to the right, will shift to the left, or it will not be affected). O It will shift to the right. O It will shift to the left. O It will not be affected.
7.B Consider the chemical equation C(s) + 2A(g) 5 2B(I) + heat. Be sure to briefly JUSTIFY each answer below. (a) Will SQUEEZING the container cause a disturbance to equilibrium? If so, then in what direction will the reaction occur? (b) Will RAISING THE TEMPERATURE of the system cause a disturbance to equilibrium? If so, then in what direction will the reaction occur? (c) What is the sign of the standard reaction ENTHALPY? Does the enthalpy change provide a favorable or unfavorable contribution to the spontaneity of the forward reaction at standard state conditions? (d) What is the sign of the standard reaction ENTROPY? Does the entropy change provide a favorable or unfavorable contribution to the spontaneity of the forward reaction at standard state conditions? (e) Based on (c,d) describe the preference for products or reactants at equilibrium at very LOW temperatures. (f) Based on (c,d) describe the preference for products or reactants at equilibrium at very HIGH temperatures.
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According to LeChatelier's principle, when the reaction quotient is less than the equilibrium constant of a reaction, the reaction: A must shift toward products to reach equilibrium. B must shift toward reactants to reach equilibrium. (c) results in an increase in standard enthalpy of formation of reactants. results in an increase in standard enthalpy of formation of products.
Calculate the value of Kp for the equation C(s) + CO₂(g) = 2 CO(g) given that at a certain temperature Kp = Kp = ? C(s) + 2 H₂O(g) = CO₂(g) + 2 H₂(g) H₂(g) + CO₂(g) = H₂O(g) + CO(g) Kpl = 3.93 = 0.769 Kp2 =
Which of the following statement is NOT true? The equilibrium constant of a reaction varies with temperature. In most biochemical systems, enthalpy is equivalent to heat. Any deviation from equilibrium prompts a process to restore the system to equilibrium. Free energy changes can be calculated from reactant and product concentrations. If a system maintains a steady state it must have reached equilibrium.
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For the reversible reaction: N 2 (g)+ O 2 (g) = 2 NO (g) AH= 181 kJ (a) What will happen to the concentrations of NO at equilibrium if O, is added? (b) What will happen to the concentrations of NO at equilibrium if NO is removed? (c) What will happen to the concentrations of NO at equilibrium if the volume of the reaction vessel is increased? (d) What will happen to the concentrations of NO at equilibrium if the temperature of the system is decreased? (e) What will happen to the concentrations of N,, 0,, and NO at equilibrium if a catalyst is added?
For a certain chemical reaction, the standard Gibbs free energy of reaction at 30.0 °C is -61.4 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 x10 S
The equilibrium constant for the reaction 2 N2(g) + 5 O2(g) ⇆ 2 N2O5(g) was measured at two temperatures: Temperature, K Kp 343 2.5x10−8 944 7.6x10−6 What is ΔHo for the reaction (in kJ/mol)?
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