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 _______

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-.

Calculate the molar solubility of AgCl in 0.020 M of AgNO3. Ksp of AgCl is 1.6 x 10-10. What is the correct Ksp equation for this reaction?