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For the reaction H_2(g) + S(g) H_2S(g) the initial concentrations are 0.060 M H_2, 0.080 MS,...
For the unbalanced reaction H2(g)+NO(g) ---> H2O(g)+N2(g): the initial concentrations are 5.25 M H2, 9.00 M...
For the unbalanced reaction H2(g)+NO(g) ---> H2O(g)+N2(g): the initial concentrations are 5.25 M H2, 9.00 M NO, and no H2O or N2. At equilibrium, [N2] = 1.75 M. A) Balance the equation using lowest-whole-number coefficients. Be sure to include states of matter in your equation. B) Calculate the value of K under the reaction conditions at equilibrium.
Consider the reaction below. The initial concentration of KBr is 0.0183 M, and the initial concentrations...
Consider the reaction below. The initial concentration of KBr is 0.0183 M, and the initial concentrations of K+ and Br− are each 0 M. If the equilibrium constant is Kc=7.76 under certain conditions, what is the equilibrium concentration of KBr? KBr(aq)⇌K+(aq)+Br−(aq) Remember to use correct significant figures in your answer (round your answer to the nearest hundredth).
The initial concentrations of L, and I in the reaction below are each 0.0401 M. If...
The initial concentrations of L, and I in the reaction below are each 0.0401 M. If the initial concentration of I, is 0.0 M and the equilibrium constant is K. 0.25 under certain conditions, what is the equilibrium concentration (in molarity) of 12 I, (aq) = L(aq) +T" (aq) • Your answer should include two significant figures.
Consider the following reaction: H_2 (g) + I_2 (g) Equilibrium 2 HI (g) Complete the following...
Consider the following reaction: H_2 (g) + I_2 (g) Equilibrium 2 HI (g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. Part A Find K_c at 25 degree C. Express your answer using three significant figures. K_c = _______ Part B Find [H_2] at 340 degree C. Express your answer using two significant figures. [H_2] = _______ M Part C Find [HI] at 445 degree C. Express your answer using three significant figures. [HI] =...
The following reaction 2H_2S(g) 2H_2(g) + S_2(g), K_c = 1.67 times 10^-7 at 800degreeC is carried...
The following reaction 2H_2S(g) 2H_2(g) + S_2(g), K_c = 1.67 times 10^-7 at 800degreeC is carried out at the same temperature with the following initial concentrations: [H_2S] = 0.100M, [H_2] = 0.100M, and [S_2] = 0.00 M. Find the equilibrium concentration of S_2. Express the molarity to three significant figures.
Consider the reaction and associated equilibrium constant. aA(g)⇌bB(g)Kc=2.0 A.) Find the equilibrium concentrations of A and...
Consider the reaction and associated equilibrium constant.
aA(g)⇌bB(g)Kc=2.0
A.) Find the equilibrium concentrations of A and B for
a = 1 and b = 1. Assume that the initial
concentration of A is 1.0 M and that no B is present at the
beginning of the reaction.
B.) Find the equilibrium concentrations of
A and B for a = 2 and b = 2. Assume that the
initial concentration of A is 1.0 M and that no B is present...
PCl_5 decomposes according to the equation PCl_5(g) doubleheadarrow PCl_3(g) + Cl_2(g) At 700 K, a 2...
PCl_5 decomposes according to the equation PCl_5(g) doubleheadarrow PCl_3(g) + Cl_2(g) At 700 K, a 2 liter flask initially contained only 0.4600 mol PCl_3(g) and 0.6875 mol PCl_5(g). After reaching equilibrium, 0.00800 mol Cl_2(g) was measured in the flask. Calculate the equilibrium concentrations of the three gases and K_c for the reaction. For the reaction, 2 H_2S(g) 2 H_2(g) + S_2 (g), K_0 = 1.7 times 10^-7 at 800.0 degree C If the initial concentration of H_2S in a closed...
Calculate Kc for the following reaction given the following equilibrium concentrations of H2(g) = 1.60 M...
Calculate Kc for the following reaction given the following
equilibrium concentrations of
H2(g) = 1.60 M CO(g) = .0030 M, and H2O(g) = 0.030 M. C(s) +
H2O(g) = CO(g) + H2(g)
(Hint: You DO include H2O(g) in the equilibrium expression)
K = ?
Save Answer Calculate K, for the following reaction given the following equilibrium concentrations of H2(9) = 1.60 M COO) = .0030 M, and H,00 = 0.030 M. Co+H,09 = COO + H2(9) (Hint: You Do include H,0...
Be sure to answer all parts. The equilibrium constant K_c for the reaction H_2(g) + Br_2(g)...
Be sure to answer all parts. The equilibrium constant K_c for the reaction H_2(g) + Br_2(g) = 2HBr(g) is 2.180 Times 10^6 at 730DegreeC. Starting with 5.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H_2, Br_2, and HBr at equilibrium. [H_2] = M [Br_2] = M [HBr] = M
A 0.060-kg tennis ball, moving with a speed of 5.50 m/s , has a head-on collision...
A 0.060-kg tennis ball, moving with a speed of 5.50 m/s , has a head-on collision with a 0.080-kg ball initially moving in the same direction at a speed of 3.54 m/s . Assume that the collision is perfectly elastic. Part A Determine the speed of the 0.060-kg ball after the collision. Express your answer to two significant figures and include the appropriate units. Part A: Part A Determine the speed of the 0.060-kg ball after the collision. Express your...
The initial concentrations of L, and I in the reaction below are each 0.0401 M. If the initial concentration of I, is 0.0 M and the equilibrium constant is K. 0.25 under certain conditions, what is the equilibrium concentration (in molarity) of 12 I, (aq) = L(aq) +T" (aq) • Your answer should include two significant figures.
Consider the following reaction: H_2 (g) + I_2 (g) Equilibrium 2 HI (g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. Part A Find K_c at 25 degree C. Express your answer using three significant figures. K_c = _______ Part B Find [H_2] at 340 degree C. Express your answer using two significant figures. [H_2] = _______ M Part C Find [HI] at 445 degree C. Express your answer using three significant figures. [HI] =...
The following reaction 2H_2S(g) 2H_2(g) + S_2(g), K_c = 1.67 times 10^-7 at 800degreeC is carried out at the same temperature with the following initial concentrations: [H_2S] = 0.100M, [H_2] = 0.100M, and [S_2] = 0.00 M. Find the equilibrium concentration of S_2. Express the molarity to three significant figures.
Consider the reaction and associated equilibrium constant.
aA(g)⇌bB(g)Kc=2.0
A.) Find the equilibrium concentrations of A and B for
a = 1 and b = 1. Assume that the initial
concentration of A is 1.0 M and that no B is present at the
beginning of the reaction.
B.) Find the equilibrium concentrations of
A and B for a = 2 and b = 2. Assume that the
initial concentration of A is 1.0 M and that no B is present...
PCl_5 decomposes according to the equation PCl_5(g) doubleheadarrow PCl_3(g) + Cl_2(g) At 700 K, a 2 liter flask initially contained only 0.4600 mol PCl_3(g) and 0.6875 mol PCl_5(g). After reaching equilibrium, 0.00800 mol Cl_2(g) was measured in the flask. Calculate the equilibrium concentrations of the three gases and K_c for the reaction. For the reaction, 2 H_2S(g) 2 H_2(g) + S_2 (g), K_0 = 1.7 times 10^-7 at 800.0 degree C If the initial concentration of H_2S in a closed...
Calculate Kc for the following reaction given the following
equilibrium concentrations of
H2(g) = 1.60 M CO(g) = .0030 M, and H2O(g) = 0.030 M. C(s) +
H2O(g) = CO(g) + H2(g)
(Hint: You DO include H2O(g) in the equilibrium expression)
K = ?
Save Answer Calculate K, for the following reaction given the following equilibrium concentrations of H2(9) = 1.60 M COO) = .0030 M, and H,00 = 0.030 M. Co+H,09 = COO + H2(9) (Hint: You Do include H,0...
Be sure to answer all parts. The equilibrium constant K_c for the reaction H_2(g) + Br_2(g) = 2HBr(g) is 2.180 Times 10^6 at 730DegreeC. Starting with 5.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H_2, Br_2, and HBr at equilibrium. [H_2] = M [Br_2] = M [HBr] = M
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