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

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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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