The equilibrium constant is 16 for the gas phase reaction: H2(g) + CO2(g) ----->

Question

The equilibrium constant is 16 for the gas phase reaction: H2(g) + CO2(g) -----> H2O(g) + CO(g). If 4.0 moles each of H2 and CO2 are placed in an empty 1.0 liter container at this temperature, what will be the equilibrium concentration of H2O in moles per liter?

Calculate the [OH- ] present in a solution labeled 1.31 M hydroxylamine. Kb for hydroxylamine is 1.1 x 10-8 . NH2OH(aq) + H2O(l) -----> NH2OH2 + (aq) + OH- (aq)

Calculate the [OH- ] present in a solution labeled 1.31 M hydroxylamine. Kb for hydroxylamine is 1.1 x 10-8 . NH2OH(aq) + H2O(l) ------> NH2OH2 + (aq) + OH- (aq)

Calculate the pH of a solution which is 0.73 M benzoic acid. HC7H5O2(aq) ----> H + (aq) + C7H5O2 - (aq) Ka = 6.5 x 10^-5

Write balanced equations for the following reactions. a) BH3 + NH3 ----> (Lewis acid-base reaction)

b) the ionization of the weak base (CH3)2NH in water

c) the stepwise ionization of H2SO4 (Two equations)

Write the chemical equation for the reaction of HCl with H2O. Based on your equation, identify each reagent (reactants and products where appropriate) as an acid or base according to each theory below. In each case, explain your reasoning.

a) Arrhenius concept

b) Bronsted-Lowry concept

c) Lewis concept

Explanation / Answer

The equilibrium constant is 16 for the gas phase reaction: H2(g) + CO2(g) ----->

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