For the reaction provided, the rate of disappearance of IO3–(aq) at a particular time and concentration is 2.6 × 10-3 mol/L·s. IO3–(aq) + 5I–(aq) + 6H+(aq) → 3I2(aq) + 3H2O(l) What is the relative rate of appearance of I2(aq)?

A 2.5 L flask is filled with 0.25 mol SO3, 0.20 mol SO2, and 0.40 mol O2, and allowed to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc = 0.12. Predict the effect on the concentration of SO3 as equilibrium is achieved by using Q, the reaction quotient. 2 SO3(g) 2 SO2(g) + O2(g)

A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B. Gas A decomposes according to the following reaction: 3A  2B + C The equilibrium concentration of gas C is 0.134 mol/L. Determine the value of the equilibrium constant, Kc.

For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 4.0 at 228°C. If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl5(g) is 0.19 M, what is the equilibrium concentration of PCl3?

Molecules must overcome a barrier called the activation energy if they are to react. The highest energy point reached during the progress of a reaction is called the ____.

The following data were obtained in a kinetics study of the hypothetical reaction A + B + C → products. [A]0 (M) [B]0 (M) [C]0 (M) Initial Rate (10–3 M/s) 0.4 0.4 0.2 160 0.2 0.4 0.4 80 0.6 0.1 0.2 15 0.2 0.1 0.2 5 0.2 0.2 0.4 20 What is the order of the reaction with respect to C?

Consider the reaction below. 2 HF(g) H2(g) + F2(g) (Kc = 1.00 × 10–2) Given that 1.00 mol of HF(g), 0.241 mol of H2(g), and 0.750 mol of F2(g) are mixed in a 5.00 L flask, determine the reaction quotient, Q.

Given the following chemical equilibria,   N2(g) + O2(g) 2 NO(g) K1   N2(g) + 3 H2(g) 2 NH3(g) K2   H2(g) + 1/2 O2(g) H2O(g) K3 Determine the method used to calculate the equilibrium constant for the reaction below.   4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) K c

Write the expression for Kp for the reaction below. 2 NOBr(g) 2 NO(g) + Br2()

The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows.   N2(g) + 3 H2(g) 2 NH3(g) ΔH = –92.2 kJ Given a system that is initially at equilibrium, which of the following actions cause the reaction to proceed to the left?