The rate for the reaction H2 (g) + Br2 (g) 2 HBr (g)is first order in both H2 and Br2 concentrations, and the rate constant k at 287 \deg C is 5.87\times 10-4 L mol-1 s-1. Suppose 1.00 L of H2 (g) at a concentration of 6.60\times 10-2 M is rapidly mixed with the same volume of Br2 (g) also at a concentration of 6.60\times 10-2 M. Calculate the time (in seconds) required for the H2 concentration to decrease to a value of 2.55\times 10-2 M. (Enter your answer to three significant figures.)

SO2 Cl2 decomposes in the gas phase by the reaction SO, Cla (9) S02 (g) + Ch(9). Part A The reaction is first order in SO2 Ca and the rate constant is 3.0 x 106 s1 at 600 K. A vessel is charged with 3.0 atm of SO2 Ch at 600 K. The partial pressure of SO, Cl, at 3.0 x 10 s is atm. 1.2 O 0.81 O 1.1 x 105 2.7 0.23

The rate constant for the first order reaction below is k = 3.3 x 10² min1 at 57 K. What is the half-life for this reaction at 57 K? A --> B+C

The first-order rate constant for the decomposition of N2O5, 2N2O5 (g)→4NO2(g) + O2 (g) Part A at 70° C is 6.82 × 10¬3 s. Suppose we start with 2.60x10-2 mol of N2O5 (g) in a volume of 2.5 L. How many moles of N2O5 will remain after 4.0 min ? Express the amount in moles to two significant digits.

In a steady-state approximation, it is assumed that     the concentrations of the reactants remain constant and small throughout the reaction.     the concentration of the product remains constant and large throughout the reaction.     The concentration of the product remains unchanged and small throughout the reaction.     the concentration of the reaction intermediates remains constant and small throughout the reaction.   there is no more information that is needed for this question.

The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H,O2(aq)H,0() + ½ O2(g) is first order in H20, with a rate constant of 1.10x10-3 min!. If the initial concentration of H,O, is 6.48×10-2 M, the concentration of H,O, will be 1.17x10-2 M after min have passed.

The gas phase decomposition of sulfuryl chloride at 600 K SO₂ Cl₂ (g) → SO₂ (g)+ Cl₂ (g) is first order in SO₂ Cl2 with a rate constant of 2.80 × 10-³ min-¹. If the initial concentration of SO₂ Cl2 is 0.00164 M, the concentration of SO₂ Cl2 will be 0.000364 M after min have passed.

The decomposition of N»Os(g) to NO2(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is: A[N,05] Rate = *[N,Os] At where k = 3.4 x 10-5 s-l at 25°C, what is the initial rate of reaction at 25°C where [N2O5]o = 4.1 x 10-2 M? а. 1.4x 10-6 mol/L's b. 3.4 x 10-5 mol/L's О с. 8.3 х 10-4 mol/L s d. 4.1 x 10-2 mol/L's e. none of these

1)The reaction A -> product 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?     2) consider the following reaction at equilibrium.2CO2 (g) ->_<-- 2CO (g) + O2 (g)  H° = -514 kJLe Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________.

he rate law for the reaction between hydrogen and nitric oxide to form nitrogen and water is rate INOPH>P What is the order vith respect to nitric oxide?