If a certain rate law for a reaction were: Rate=k [A]2[B]/[C]1/2 What would the rate be if the [A] were octupled (8x), [B] were duodecupled (12x), and [C] were nonupled (9x)?

The rate law for the reaction is below: rate = k[IO3 ]²[SO3²]⁹ What is the meaning of the coefficients p and q in the reaction? They represent the coefficients in the balanced equation. They represent the rate each compound is used. They represent the charge on the ions. They represent the order of reaction with respect to each reactant.

please help me with question a and b only

we now have: Step 1: Fast, reversible HA = H+ + A- Step 2: Fast, reversible X + H+ = HX+ Step 3: Slow HX+ = productsrate= k3 k2/k-2 [X][HX+]   Does the current rate law contain an intermediate?

How do I answer number 28?

Given the following rate law: rate = k [AJ? [B]° [C] What happens to the rate if: The concentration of C is tripled? v Select Decreases by a factor of 4 Decreases by a factor of 2 Increases by a factor of 4 Increases by a factor of 8 The concentration of A is halved? The concentration of B is doubled? The rate decreases The rate increases The temperature of the reaction is The rate stays the same increased? Increases by a factor of 3 Increases by a factor of 2

23. Consider the following reaction: 2 NO2(g) + O3(g)  N2O5(g) + O2(g) (a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)]     Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO2(g)] = 0.530 M and [O3(g)] = 1.08 M?Rate =_____  M/s.(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.06 M while the concentration of O3(g) is 1.08 M?Rate =____  M/s

9:21 < A) s-¹ B) M-¹s-¹ The reaction, 2 NO(g) + O₂(g) → 2 NO₂(g) has a rate law, rate = k{NO] [O₂]. If the rate of the reaction is 0.60 M/s when [NO] is 1.5 M and [O₂] is 2.0 M, what are the units of the rate constant, k? C) Ms-¹ Question 5 of 20 D) M-²S-¹ E) None of these. 11 Tap here or pull up for additional resources Submit

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,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.620 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 24.0 M / s when [N2] = 1.5 M and [H2] = 0.16 M. Calculate the value of the k = |M -2 -1 •S rate constant. Round your answer to 2 significant digits.