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Question 9 The equilibrium constant (K) of the following reaction is 2.85×10-5 at 100.0 K. What is the value of the equilibrium constant, K? CO₂(g) + 3 H₂(g) = CH4(g) + H2₂O(g) K = Question 10 The equilibrium constant (K) is 3.0×102 for the following reaction: CS₂(g) + 4H₂(g) = CH₂(g) + 2 H₂S(g) [CS₂] = 0.25 atm [H₂] = 0.50 atm [CH] = 0.0015 atm [H₂S] = Type numbers in the boxes. 10 points Calculate the partial pressure of H₂S at equilibrium, if the concentrations of the other species are determined to be: atm Type numbers in the boxes. 10 points Concentrations of each species at 300 K for the following reaction were measured and are given in the table below. Question 6 H₂(g) + I2(g) = 2 HI(g) Q Question 7 Species Calculate the value of Q at 300 K. Question 8 H₂ L₂ K = HI 0.205 Concentration (M) 0.165 0.25 Ke Fill in the following blanks based on the given information. In order for the reaction to reach equilibrium, the concentration of the will increase. = 0.290 at 300 K What is the value of the equilibrium constant, K K₂? Type numbers in the boxes. 10 points The equilibrium constant (K) of the following reaction is 3.933 at 298 K. Type numbers in the boxes. 10 points CO₂(g) + 3 H₂(g) = CH4(g) + H₂O(g) Fill in the blanks by selecting one option from each menu. 3 points

Question 9 The equilibrium constant (K) of the following reaction is 2.85×10-5 at 100.0 K. What is the value of the equilibrium constant, K? CO₂(g) + 3 H₂(g) = CH4(g) + H2₂O(g) K = Question 10 The equilibrium constant (K) is 3.0×102 for the following reaction: CS₂(g) + 4H₂(g) = CH₂(g) + 2 H₂S(g) [CS₂] = 0.25 atm [H₂] = 0.50 atm [CH] = 0.0015 atm [H₂S] = Type numbers in the boxes. 10 points Calculate the partial pressure of H₂S at equilibrium, if the concentrations of the other species are determined to be: atm Type numbers in the boxes. 10 points Concentrations of each species at 300 K for the following reaction were measured and are given in the table below. Question 6 H₂(g) + I2(g) = 2 HI(g) Q Question 7 Species Calculate the value of Q at 300 K. Question 8 H₂ L₂ K = HI 0.205 Concentration (M) 0.165 0.25 Ke Fill in the following blanks based on the given information. In order for the reaction to reach equilibrium, the concentration of the will increase. = 0.290 at 300 K What is the value of the equilibrium constant, K K₂? Type numbers in the boxes. 10 points The equilibrium constant (K) of the following reaction is 3.933 at 298 K. Type numbers in the boxes. 10 points CO₂(g) + 3 H₂(g) = CH4(g) + H₂O(g) Fill in the blanks by selecting one option from each menu. 3 points

Chemistry
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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Question 9 The equilibrium constant (K) of the following reaction is 2.85×10-5 at 100.0 K. What is the value of the equilibrium constant, K? CO₂(g) + 3 H₂(g) = CH4(g) + H2₂O(g) K = Question 10 The equilibrium constant (K) is 3.0×102 for the following reaction: CS₂(g) + 4H₂(g) = CH₂(g) + 2 H₂S(g) [CS₂] = 0.25 atm [H₂] = 0.50 atm [CH] = 0.0015 atm [H₂S] = Type numbers in the boxes. 10 points Calculate the partial pressure of H₂S at equilibrium, if the concentrations of the other species are determined to be: atm Type numbers in the boxes. 10 points
Transcribed Image Text:Question 9 The equilibrium constant (K) of the following reaction is 2.85×10-5 at 100.0 K. What is the value of the equilibrium constant, K? CO₂(g) + 3 H₂(g) = CH4(g) + H2₂O(g) K = Question 10 The equilibrium constant (K) is 3.0×102 for the following reaction: CS₂(g) + 4H₂(g) = CH₂(g) + 2 H₂S(g) [CS₂] = 0.25 atm [H₂] = 0.50 atm [CH] = 0.0015 atm [H₂S] = Type numbers in the boxes. 10 points Calculate the partial pressure of H₂S at equilibrium, if the concentrations of the other species are determined to be: atm Type numbers in the boxes. 10 points
Concentrations of each species at 300 K for the following reaction were measured and are given in the table below. Question 6 H₂(g) + I2(g) = 2 HI(g) Q Question 7 Species Calculate the value of Q at 300 K. Question 8 H₂ L₂ K = HI 0.205 Concentration (M) 0.165 0.25 Ke Fill in the following blanks based on the given information. In order for the reaction to reach equilibrium, the concentration of the will increase. = 0.290 at 300 K What is the value of the equilibrium constant, K K₂? Type numbers in the boxes. 10 points The equilibrium constant (K) of the following reaction is 3.933 at 298 K. Type numbers in the boxes. 10 points CO₂(g) + 3 H₂(g) = CH4(g) + H₂O(g) Fill in the blanks by selecting one option from each menu. 3 points
Transcribed Image Text:Concentrations of each species at 300 K for the following reaction were measured and are given in the table below. Question 6 H₂(g) + I2(g) = 2 HI(g) Q Question 7 Species Calculate the value of Q at 300 K. Question 8 H₂ L₂ K = HI 0.205 Concentration (M) 0.165 0.25 Ke Fill in the following blanks based on the given information. In order for the reaction to reach equilibrium, the concentration of the will increase. = 0.290 at 300 K What is the value of the equilibrium constant, K K₂? Type numbers in the boxes. 10 points The equilibrium constant (K) of the following reaction is 3.933 at 298 K. Type numbers in the boxes. 10 points CO₂(g) + 3 H₂(g) = CH4(g) + H₂O(g) Fill in the blanks by selecting one option from each menu. 3 points
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