The reaction A + B 2 C has the rate law rate = K[A] [B]³. By what factor does the rate of reaction increase when [A] remains constant but [B] is doubled?

The reaction A + 2 B → C has the rate law rate = k[A][B]. By what factor does the rate of reaction increase when both [A] and [B] are doubled?

So how can I tell the difference if the rate is increasing or decrease? I know it’s doubling but in what direction? And what would be the correct answer ?

What is the overall reaction order for the following rate law: Rate = k[A][B][C]²

Propose a reaction pathway consisting of only a unimolecular or bimolecular steps for the 2A+B-->C+D that is consistent with the rate law rate=k(A)(B). Make sure you label which step is the rate determining step and prove that your proposed mechanism gives both the overall reaction and overall rate law. Explain the assumptions you must make in order for your mechanism to be consistent with the actual rate law.

The rate equation for the reaction A→B + C is expressed in the forms of rate of disappearance of A = k[A]x. The value of the rate constant is 0.100(units unspecified) and [A]= 0.050 mol/L. What are the units of k and the rate reactions in mol/L-s if the reaction is first order? a. k = 0.1 /s, r = 0.0040 M/s b. k = 0.2/s, r = 0.0060 M/s c. k = 0.1 /s, r = 0.0050M/s d. k = 0.2 M/s, r = 0.0070 M/s

Consider the reaction and its rate law. 3A+3B⟶productsrate=?[A][B]2 What is the order with respect to A?

If tripling the concentration of a single reactant R in a multi-reactant reaction (while leaving all other conditions unchanged) leads to a nine-fold increase in rate, it can be deduced * O that the complete rate law is Rate= k[R] O that the complete rate law is Rate= k[R]^2 O that the complete rate law is Rate= k[R]^3 that the complete rate law is Rate= k[R]^9 only that the order with respect to [R] is 2

A value of k is found from the rate equation Rate = k[A]m[B]n. If m=1 and n=4 and -1 the unit for the initial rate is M/h. The unit of k is found to be MX h-¹ (M to the power of x h to the power of minus 1). What is the value of x?

Suggest a mechanism behind the reaction    NO(g) + Cl2(g)  à  NOCl(g)  + Cl(g) with the rate law    rate = k [NO]2 [Cl2]   This reaction cannot be a one step reaction because of its rate law. It is therefore a multistep reaction, where the slow step represents a reaction between 2 molecules of NO with one molecule of Cl2                 (slow)       2NO   +   Cl2    à   ……….                  (fast).                                à  …………                                NO     +     Cl2.     à    NOCl    +    Cl