Given the equilibrium constants for the following two reactions in aqueous solution at 25 °C, HF(aq) ↔ H+(aq) + F–(aq)                       Kc = 6.8 × 10–4 H2C2O4(aq) ↔ 2 H+(aq) + C2O42–(aq)     Kc = 3.8 × 10–6 determine the value of Kc for the reaction: 2 HF(aq) + C2O42–(aq) ↔ 2 F–(aq) + H2C2O4(aq) Should the second equation be changed and if so how?

Predict the direction of spontaneity (ΔG) by stating is it spontaneous, nonspontaneous, or at equilibrium for iron(III) oxide decomposing to iron and oxygen

Using the data in the table below answer the following questions about the reaction: A  +  B  →  P What is the rate constant, k?

In the process of balancing the following equation by the method of half-reactions  ClO3- (aq) + NO (g) –> Cl2 (g) + NO3- (aq) (acidic solution) When the cell is balanced how many electrons are in the reaction?

Complete and balance the following equation by the method of half-reactions Cr(OH)3(s) + ClO–(aq) → CrO42–(aq) + Cl2(g) (basic solution) When the two cells are combined how many hydroxide (OH-) are in the cell?

In calculating ΔH°, ΔS°, and ΔG° at 400 K for the reaction 2 SO2(g) + O2(g) → 2 SO3(g) Assume ΔH°, ΔS° do not change with temperature What is ΔG° for the SO2(g)?

A student prepared a {x} M solution of formic acid (HCOOH) and found its pH at 25 °C to be {y}. Calculate Ka for formic acid at this temperature.

Determine ΔHf⁰, ΔS⁰, and ΔGf⁰ for the following reaction. HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) What is the ΔGf⁰ of HCl (aq)?

What is the pH of a 0.0037 M solution of H2CO3?  H2CO3 (aq) ↔ H+ (aq) + HCO3- (aq)             Ka1 = 4.3 × 10–7 HCO3- (aq) ↔ H+ (aq) + CO32- (aq)               Ka2 = 5.6 × 10–11

The Kb of cyanide ion (CN-) is 2.0 × 10-5 at 25.0°C. Calculate the pOH of a 0.20 M solution of CN-. Complete the ICE table (use commas to separate answers values and x only you do not need to label the compounds). Initial  _______ Change _______ Equilibrium _______