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Consider the following equilibrium: CO(g) + H2O(g) ⇌ H2(g) + CO2(g)   Kc = 16 Suppose that 2.00 mol of CO  and 2.00 mol of H2O are placed in 0.500 L flask and allowed to come to equilibrium at high temperature. A) Calculate the equilibrium concentration of CO2(g) [a] mol/L B) Calculate the equilibrium concentration of H2O (g) [b] mol/L C) Calculate the equilibrium concentration of H2(g) [c] mol/L D) Calculate the equilibrium concentration of CO (g) [d] mol/L

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.00 at 25°C.

Select the conjugate base of the following acids:

The strongest intermolecular interaction between CBr4 molecules arise from ______

A 0.300 M solution of a weak base, B, has a pH of 9.75. Calculate the value of Kb for the base. Hint: Write the reaction between the base B and water (B + H2O → BH+ + OH-), and use on ICE Table. You must show all of your work for credit.

Predict the sign (∆S > 0 or ∆S < 0) of the entropy change (∆S) for the following processes. (a) Pb2+(aq) + S2-(aq) ⟶ PbS(s) [a] (b) NaNO3(s) ⟶ Na+(aq) + NO3-(aq) [b] (c) CO2(s) ⟶ CO2(g)[c]

Determine the standard entropy change (∆So) for this reaction. 2KCl(s) ⟶2K(s) + Cl2(g) Substance (state) So (J/mol.K) KCl(s) 82.6 K(s) 64.7 Cl2(g) 223.1

Are the following solutions acidic, basic, or neutral? a) Ba(NO3)2(aq) [a] b) NH4Cl(aq) [b] c) NaClO(aq) [c]

Calculate ∆Go for the following reaction at 298 K. CH3OH(g)  ⇌ CO(g) + 2H2(aq)    Kc = 7.1 x 10-6

For the reaction A + 3B → 2C, how does the rate of disappearance of B compare to the rate of production of C?