Consider the following equilibrium reaction: H2CO3 (aq)  ⇌  H+ (aq) + HCO3– (aq);     K = 5.0 x 10–7  If the initial concentrations of the species are: [H2CO3] = 0.100 M;   [H+] = 2.00 x 10–5 M;   [HCO3–] = 2.00 x 10–3 M Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change?   Select one: a. Q = K, so the reaction is at equilibrium. b. Q > K, so the reaction moves to the right. c. Q < K, so the reaction moves to the right. d. Q < K, so the reaction moves to the left. e. Q > K, so the reaction moves to the left.

Using the law of mass action, write the equilibrium expression for each of the following reactions. (a) 8 H2(g) + Sg(s) 2 8 H,S(g) (b) C(s) + H,O(€) + Cl2(g) = COCl,(g) + H,(g) (c) CaCO3(s) 2 CaO(s) + CO2(g) (d) 3 C,H2(g) = CH(t) Acti

1. Write the equilibrium constant expressions Ke for the following reactions. a) CHa(g) + H20 (g) →CO(g) + 3 H2 (g) b) 2 N2H4 (I) + 2 NO2 (g) → 3 N2 (g) + 4 H2O (I) c) NHẠNO3 (s) 2 H20 (g) + N20 (g) d) 4 HCl (aq) + MnO2 (s) = MnCl2 (aq) + 2 H2O (1) + Cl2 (g) e) Ca3(PO4)2 (s) = 3 Ca²* (aq) + 2 PO,³- (aq)

Hydrofluoric acid and water react to form fluoride anion and hydronium cation, like this: + HF(aq)+H,O(1)→F (aq)+H;O"(aq) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing an aqueous solution of hydrofluoric acid, water, fluoride anion, and hydronium cation at equilibrium has the following composition: compound amount HF 2.21 g H,0 857. g F 0.169 g H;O 0.141 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0

Explain everything please

A 2.21-L vessel was found to contain 4.18 x 10 -2 mol of CO 2, 2.81 x 10 -2 mol of CO, and 8.89 x 10 -3 mol of O 2 at 298 K. Is the system at equilibrium for the reaction 2CO 2 ⇌  2CO + O 2? If not, which direction must the reaction proceed to achieve equilibrium? ( Keq = 1.2 x 10 -13)

The equilibrium constant (Kc) for this reaction is 1.60 at 990 °C:H2(g) + CO2(g) ⇌ H2 O(g) + CO(g)Calculate the number of moles of each component in the final equilibrium mixture obtained from adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00-L container at 990 °C.

Carbon monoxide and water vapor are formed when carbon dioxide and hydrogen react. CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium constant for the reaction is KC = 2.10 at 247 ℃. If 0.657 mol of carbon dioxide is added to 0.512 mol of hydrogen in a 0.84–L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of carbon dioxide? Report your answer to THREE significant figures.

The equilibrium constant, K eq , for the reaction:SO 3 (g) + NO (g) ⇋ NO 2 (g) + SO 2 (g)was found to be 0.500 at a certain temperature. If 0.300 mol of SO 3 and 0.300 mol NOwere placed in a 2.00 L container and allowed to react, what would be the equilibriumconcentration of each gas? Include an ICE table

The equilibrium constant (Kc) for the reaction PCl3 (g) + Cl₂ (g) ⇒ PC15 (9) equals 49 at 230°C℃. If 0.319 mol each of phosphorus trichloride and chlorine are added to a 4.90 L reaction vessel, what is the equilibrium composition of the mixture at 230°C? mol PC13 mol Cl₂ mol PC15