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?

Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 °C, Kc equals 1.0 × 10−5.   N2(g) + O2(g) 2 NO(g)   If 0.030 mol N2 and 0.030 mol O2 are sealed in a 1.0 L flask at 1500 °C, what is the concentration of NO(g) when equilibrium is established?

The equilibrium constant (Kc) for the decomposition of ammonium hydrogen sulfide, NH4HS(s)  NH3(g) + H2S(g), is 1.8 × 10–4 at 25 °C. If excess NH4HS(s) is allowed to equilibrate at 25 °C, what is the equilibrium concentration of NH3?