Are there more reactants or products present in this initial system? How can you tell?
The following equilibrium is observed:
Co(H2O)62+(aq) + 4 Cl-(aq) <=> CoCl42-(aq) + 6 H2O(g)
The Co(H2O)62+ complex is pink, and the CoCl42- complex is blue.
Are there more reactants or products present in this initial system? How can you tell?
How is a reversible chemical reaction at equilibrium affected by adding more reactants to this system, removing products from the system, or changing the temperature of the system?
12. The pKa of NH4+ is 9.8 and the pka of H2O is 15.7 Would this reaction have more products or reactants at equilibrium? NH3 + H2O - NH4+ + OH A. Reactants B. Products C. Equal amounts D. Can't tell from this information
How can a reaction which favors reactants at equilibrium be driven to generate additional products? I am confused, how can you generate additional products if the equilibrium constant for this reaction is < 1, doesn't K need to be > 1 to generate additional products?
for the following values of k indicate whether the products or reactants are present in larger amounts 10 0.00000079 © 10000000 6 0.004s Products or reactants?
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] =...
Question 15 3 pts Are there more reactants, more products, or about equal amounts when the reaction between hypochlorous acid and pyridine reaches equilibrium? HCIO(aq) + CsHsN(aq) = O about equal amounts O reactants O products
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (d) 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) KP = 16.5; initial pressures: SO3 = 1.00 atm, SO2 = 1.00 atm, O2 = 1.00 atm (e) 2NO(g) + Cl2 (g) ⇌ 2NOCl(g) Kc = 4.6 × 104 ; [NO] = 1.00 M, [Cl2] = 1.00...
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...
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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)...