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Carbon disulfide and chlorine react according to the following equation:CS2(g) + 3Cl2(g)    S2Cl2(g) + CCl4(g)When 2.14 mol of CS2 and 5.85 mol of Cl2 are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.620 mol of CCl4. How many moles of Cl2 are present at equilibrium?

At a given temperature, a first-order reaction has a rate constant of 3.4 × 10–3 s–1. The time required for the reaction to be 44% completed is

A general reaction written as A + 2B → C + 2D is studied and yields the following data: [A]0[B]0Initial Δ[C]/Δt 0.150 M0.150 M8.00 × 10–3 mol/L·s 0.150 M0.300 M1.60 × 10–2 mol/L·s 0.300 M0.150 M3.20 × 10–2 mol/L·s What is the numerical value of the rate constant?

Please mark your paper A1.  Show your work on the free response packet and then box your answers.  Draw a reaction diagram for an endothermic reaction.  Label the following reactants products ∆Hrxn Ea transition state Show how it would change if it contained a catalyst.   

Consider the reaction represented by the equation  2SO2(g) + O2(g)  2SO3(g). For the system at chemical equilibrium, which of the following explains what happens after the addition of oxygen gas (assume constant temperature)?

The reaction 3A + 4B → products is second order in A and second order in B. What is the overall order of the reaction?

A chemical reaction that is first order in X is observed to have a rate constant of 1.7 × 10–2s–1. If the initial concentration of X is 1.0 M, what is the concentration of X after 190 s?

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 + CThe equilibrium concentration of gas C is 0.146 mol/L. Determine the value of the equilibrium constant, K.

The reaction A → products is second order. If the initial concentration of A is 0.436 M and, after 52.8 seconds have elapsed, the concentration of A has fallen to 0.0476 M, what is the rate constant of the reaction?

A general reaction written as A + 2B → C + 2D is studied and yields the following data: [A]0[B]0Initial Δ[C]/Δt 0.150 M0.150 M8.00 × 10–3 mol/L·s 0.150 M0.300 M1.60 × 10–2 mol/L·s 0.300 M0.150 M3.20 × 10–2 mol/L·s What is the order of the reaction with respect to B?