The rate constant k for the reaction shown below is 2.6 × 10–8 L/mol⋅s when the reaction proceeds at 300.0 K. The activation energy is 98000 J/mol. (The universal gas constant, R, is 8.314 J/mol·K) 2NOCl → 2NO + Cl2 What is the magnitude of the frequency factor A for the reaction?

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased

Consider the following reaction: 4 HBr(g) + O2(g)  2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate =  _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/s

The activation energy for the following reaction is 125 kJ/mol, and AE for the reaction is -216 kJ/mol. NO₂(g) + CO(g) → NO(g) + CO₂(g) What is the activation energy for the reverse reaction NO(g) + CO₂(g) → NO₂(g) + CO(g) Please enter your answer as a real number only. (The units should be kJ/mol, but leave that off. Just enter a number like 420.3. But don't enter 420.3. Enter the correct answer.)

A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0 ° C. What is the magnitude of k at 55.0°C if Ea = 55.5 kJ/mol. 1.05 103 2.67 1065 277 1.35 102 1.65 104

Consider the reaction: A(g)+1/2B(g)→2C(g) Identify the expression for the rate of the reaction with respect to each of the reactants and products.         When C is increasing at a rate of 4.0×10−2 M⋅s−1, how fast is B decreasing? Express your answer using two significant figures. How fast is A decreasing? Express your answer using two significant figures.

Calculate the rate constant, k, for a reaction at 73.0 °C that has an activation energy of 77.2 kJ/mol and a frequency factor of 2.61 x 10¹¹ s-¹. k = X10 TOOLS $1

Consider the following reaction in aqueous solution: 5Br-(aq) +BrO3-(aq) +6H+(aq)→ 3Br2(aq) + 3H2O(l) If the rate of disappearance of Br–(aq) at a particular moment during the reaction is 2.5 x 10–4 mol L–1 s–1, what is the rate of appearance of Br2(aq) at that moment?   Question 2 options:   a)  2.1 x 10–4 mol L–1 s–1   b)  1.5 x 10–4 mol L–1 s–1   c)  7.2 x 10–4 mol L–1 s–1   d)  9.4 x 10–4 mol L–1 s–1

The rate of a certain reaction is given by the following rate law: rate=k|N, || H2 K[N][H° Use this information to answer the questions below. What is the reaction order in N,? 1 х10 What is the reaction order in H2? ? 2 What is overall reaction order? 3 At a certain concentration of N, and H2, the initial rate of M reaction is 5.0 x 103 M / s. What would the initial rate of the reaction be if the concentration of N2 were halved? Round S your answer to 2 significant digits. The rate of the reaction is measured to be 0.640 M/ s when [N2] - 2 • S 1.8 M and [H2] 1.4 M. Calculate the value of the rate - 1 k = |M constant. Round your answer to 2 significant digits.

The following reaction was studied at 25°C. The following results were obtained. a) What is the rate law for this reaction at this temperature? b) What is the value of the rate constant? Be sure to include the correct units in your answer.