9. Find the equilibrium concentrations for all reactants and products in the following equilibrium reaction. The...
9. Find the equilibrium concentrations for all reactants and products in the following equilibrium reaction. The initial concentration of the N2 is 0.78M and the initial concentration of O2 is 0.21M. There is no product initially. The equilibrium constant is K = 2.36 x 10-5. If you make any assumptions you are required to prove that they were valid!
N2 + O2 yield 2 NO
The equilibrium concentration of the N2 is __________________________
The equilibrium concentration of the O2 is __________________________
The equilibrium concentration of the NO is __________________________
Homework Answers
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9. Find the equilibrium concentrations for all reactants and
products in the following equilibrium reaction. The...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) +...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + ...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. Calculate the equilibrium concentration of Cl2 in that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g)...
Select all of the true statements regarding chemical equilibrium. The concentrations of reactants and products are...
Select all of the true statements regarding chemical equilibrium. The concentrations of reactants and products are equal. The concentrations of reactants and products remain constant. Reactants are being converted to products and vice versa. The rates of the forward and reverse reactions are equal. Write the equilibrium constant expression for the reaction A(s)+3 B() 2C (aq) D(aq) in terms of [A]. [B]. [C], and [D] K = Write the equilibrium-constant expression for the reaction shown in terms of [A]. [B]....
please explain step by step. 3. Determine the equilibrium concentrations of all the reactants and products...
please explain step by step.
3. Determine the equilibrium concentrations of all the reactants and products for the equilibrium described below if you start with an initial concentration of hydrogen and nitrogen each at 6.8 x 10-2M with no HCN present. You can assume there is sufficient graphite (carbon) present to maintain an equilibrium and that the temperature is constant at 2050K. (15 points) H2(g) + Cs, graphite) + N2(g) - 2HCNG) Kc = 3.43x10-3at 2050K Initial concentrations: [H2] =...
Deriving concentrations from data The equilibrium constant, K, of a reaction at a particular temperature is...
Deriving concentrations from data The equilibrium constant, K, of a reaction at a particular temperature is detemined by the concentrations or pressures of the reactants and products at equilibrium. In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula...
Chemie Heterogeneous Reaction Chemical reactions may be envisioned in terms of reactants and products and written...
Chemie Heterogeneous Reaction Chemical reactions may be envisioned in terms of reactants and products and written in the general form A +bB - C +dD Reactants Products The equilibrium constant may be expressed in the form K - LORD up or K, - P2 where [C] represents the molar concentration of Catequilibrium. For a given reaction, the concentrations at equilibrium would have to be determined experimentally. In application, there are practical cases where some of the reactants and/or products do...
A(g) -> B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each of the...
A(g) -> B(g)+C(g) Find the equilibrium concentrations of A,
B, and C for each of the following different values of Kc. Assume
that the initial concentration of A in each case is 1.0 M and that
the reaction mixture initially contains no products.
UNITS_18_19_HW Exercise 15.61 A Review Constants 1 Peric Submit Request Answer Consider the following reaction: A(9) B(9) + C(9) Find the equilibrium concentrations of A, B, and C for each of the following different values of Ke....
At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc,...
At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction Part A aA + bB = CC + dD A mixture initially contains A, B, and C in the following concentrations: [A] = 0.350 M , [B] = 1.15 M, and [C] = 0.600 M. The following reaction occurs and equilibrium is established: where a, b, c, and d...
1. The initial concentrations or pressures of reactants and products are given for each of the...
1. The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and use it to determine the direction in which each system will proceed to reach equilibrium. Write "R" if the reactions shifts to the right towards products or "L" if it shifts left towards reactants. A. {NO} = 1.00 M, {Cl2} = 1.00 M, {NOCl} = 0.00 M; K = 4.6 x 104 2NO(g)+Cl2(g)<->2NOCl(g) B. {SO3} = 2.00...
A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all...
A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all reactants have been converted to products. all products have been removed from the reaction mixture. D) the catalyst has been used up. E) the rate of the forward reaction equals the rate of the reverse reaction. 6) An equilibrium in which all the components are gases is a A) heterogeneous equilibrium. D) homogeneous B) liquid C) catalytic E) reversible 7) The equilibrium...
Select all of the true statements regarding chemical equilibrium. The concentrations of reactants and products are equal. The concentrations of reactants and products remain constant. Reactants are being converted to products and vice versa. The rates of the forward and reverse reactions are equal. Write the equilibrium constant expression for the reaction A(s)+3 B() 2C (aq) D(aq) in terms of [A]. [B]. [C], and [D] K = Write the equilibrium-constant expression for the reaction shown in terms of [A]. [B]....
please explain step by step.
3. Determine the equilibrium concentrations of all the reactants and products for the equilibrium described below if you start with an initial concentration of hydrogen and nitrogen each at 6.8 x 10-2M with no HCN present. You can assume there is sufficient graphite (carbon) present to maintain an equilibrium and that the temperature is constant at 2050K. (15 points) H2(g) + Cs, graphite) + N2(g) - 2HCNG) Kc = 3.43x10-3at 2050K Initial concentrations: [H2] =...
Deriving concentrations from data The equilibrium constant, K, of a reaction at a particular temperature is detemined by the concentrations or pressures of the reactants and products at equilibrium. In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula...
Chemie Heterogeneous Reaction Chemical reactions may be envisioned in terms of reactants and products and written in the general form A +bB - C +dD Reactants Products The equilibrium constant may be expressed in the form K - LORD up or K, - P2 where [C] represents the molar concentration of Catequilibrium. For a given reaction, the concentrations at equilibrium would have to be determined experimentally. In application, there are practical cases where some of the reactants and/or products do...
A(g) -> B(g)+C(g) Find the equilibrium concentrations of A,
B, and C for each of the following different values of Kc. Assume
that the initial concentration of A in each case is 1.0 M and that
the reaction mixture initially contains no products.
UNITS_18_19_HW Exercise 15.61 A Review Constants 1 Peric Submit Request Answer Consider the following reaction: A(9) B(9) + C(9) Find the equilibrium concentrations of A, B, and C for each of the following different values of Ke....
At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction Part A aA + bB = CC + dD A mixture initially contains A, B, and C in the following concentrations: [A] = 0.350 M , [B] = 1.15 M, and [C] = 0.600 M. The following reaction occurs and equilibrium is established: where a, b, c, and d...
A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all reactants have been converted to products. all products have been removed from the reaction mixture. D) the catalyst has been used up. E) the rate of the forward reaction equals the rate of the reverse reaction. 6) An equilibrium in which all the components are gases is a A) heterogeneous equilibrium. D) homogeneous B) liquid C) catalytic E) reversible 7) The equilibrium...
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