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ΔGf°(I2(g)) = 19
kJ/mol
7. For the reaction H2(g) +12(g) = 2HI(g) K = 50.0 at...
H2(g) + I2(g) ⇌ 2HI(g) ΔG o for the reaction is 2.60 kJ/mol at 25°C. What...
H2(g) + I2(g) ⇌ 2HI(g) ΔG o for the reaction is 2.60 kJ/mol at 25°C. What is the minimum partial pressure of I2 required for the reaction to be spontaneous in the forward direction at 25°C if the partial pressures of H2 and HI are 4.1 and 2.05 atm, respectively?
A,) ΔG o for the reaction H2(g) + I2(g) ⇌ 2HI(g) is 2.60 kJ/mol at 25°C....
A,) ΔG o for the reaction H2(g) + I2(g) ⇌ 2HI(g) is 2.60 kJ/mol at 25°C. Calculate ΔG, and predict the direction in which the reaction is spontaneous. The initial pressures are: PH2 = 3.10 atm PI2 = 1.5 atm PHI 1.75 atm ΔG = kJ/mol b.)The reaction is spontaneous in the forward direction. The reaction is spontaneous in the reverse direction. Cannot be determined.
For the reaction H2 (g) + I2 (g) = 2HI (g); Kc =50.0. Calculate the concentration...
For the reaction H2 (g) + I2 (g) = 2HI (g); Kc =50.0. Calculate the concentration of HI (g) at equilibrium if the initial concentration of each substance is 0.0600 M and the reaction mixture is allowed to come to equilibrium. (Hint: ICE Table)
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K. A mixture of H2, I2 and HI, each at 0.020 M, was introduced into a container at 700 K. Which of the following is true? At equilibrium, [H2] = [I2] = [HI]. No net change occurs because the system is at equilibrium. The reaction proceeds to the left producing more H2(g) and I2(g). The reaction proceeds to the right producing more HI(g). At equilibrium,...
Enter your answer in the provided box. Given the reaction: H2(g) + I2(g) ⇌ 2HI(g) ΔG...
Enter your answer in the provided box. Given the reaction: H2(g) + I2(g) ⇌ 2HI(g) ΔG o for the reaction is 2.60 kJ/mol at 25degree C. What is the minimum partial pressure of I2 required for the reaction to be spontaneous in the forward direction at 2degrees C if the partial pressures of H2 and HI are 3.5 and 1.75 atm, respectively?
At 699 K, AG° = -23.25 kJ for the reaction H2(g) + 12(g) = 2 HI(g)....
At 699 K, AG° = -23.25 kJ for the reaction H2(g) + 12(g) = 2 HI(g). Calculate AG for this reaction if the reagents are both supplied at 10.0 atm pressure and the product HI is at 1.00 atm pressure. Select one: O a. -36.6 kj O b. -50.0 kj O C. -3.5 kg O d. +50.0 kJ o e. +36.6 kJ
NOLUL PULS. AGº for the reaction H2(g) +12(8) = 2HI(g) is 2.60 kJ/mol at 25°C. Calculate...
NOLUL PULS. AGº for the reaction H2(g) +12(8) = 2HI(g) is 2.60 kJ/mol at 25°C. Calculate AG, and predict the direction in which the reaction is spontanec The initial pressures are: PH, = 3.70 atm P1, = 1.5 atm Ph1 = 1.75 atm AG= The reaction is spontaneous in the forward direction. The reaction is spontaneous in the reverse direction. Cannot be determined.
Consider this reaction at 721 K: H2(g) + I2(g)
Consider this reaction at 721
K:
H2(g) + I2(g)
2HI
(g)
If we start with 1.00 Molar H 2 and 2.00 Molar
I2, what is the equilibrium concentration of HI?
Kc = 50.5 (Hint: need quadratic)
1.87 M
0.157 M
3.83 M
3.50 x 10 -4M
1.04 x 10 -3M
8.67 x 10 -6M
0.604 M
5.80
M
Given the equilibrium reaction: 2HI(g) H2(g) + I2(g) A sample mixture of HI, H2, and 12,...
Given the equilibrium reaction: 2HI(g) H2(g) + I2(g) A sample mixture of HI, H2, and 12, at equilibrium, was found to have [H2]- 1.4 x 102 Mand [HI 4.0 x 102 M. If Keq 1.0 x 10, calculate the molar concentration of I2 in the equilibrium mixture, Enter your answer in the provided box. ]= м
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) ----> H2(g)...
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) ----> H2(g) + I2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.306 M HI, 4.10×10-2 M H2 and 4.10×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.208 mol of HI(g) is added to the flask? [HI] = ______ M [H2] = ______ M [I2] = ______M
At 699 K, AG° = -23.25 kJ for the reaction H2(g) + 12(g) = 2 HI(g). Calculate AG for this reaction if the reagents are both supplied at 10.0 atm pressure and the product HI is at 1.00 atm pressure. Select one: O a. -36.6 kj O b. -50.0 kj O C. -3.5 kg O d. +50.0 kJ o e. +36.6 kJ
NOLUL PULS. AGº for the reaction H2(g) +12(8) = 2HI(g) is 2.60 kJ/mol at 25°C. Calculate AG, and predict the direction in which the reaction is spontanec The initial pressures are: PH, = 3.70 atm P1, = 1.5 atm Ph1 = 1.75 atm AG= The reaction is spontaneous in the forward direction. The reaction is spontaneous in the reverse direction. Cannot be determined.
Consider this reaction at 721
K:
H2(g) + I2(g)
2HI
(g)
If we start with 1.00 Molar H 2 and 2.00 Molar
I2, what is the equilibrium concentration of HI?
Kc = 50.5 (Hint: need quadratic)
1.87 M
0.157 M
3.83 M
3.50 x 10 -4M
1.04 x 10 -3M
8.67 x 10 -6M
0.604 M
5.80
M
Given the equilibrium reaction: 2HI(g) H2(g) + I2(g) A sample mixture of HI, H2, and 12, at equilibrium, was found to have [H2]- 1.4 x 102 Mand [HI 4.0 x 102 M. If Keq 1.0 x 10, calculate the molar concentration of I2 in the equilibrium mixture, Enter your answer in the provided box. ]= м
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