From the reaction: `CH_3Br(aq) +OH_(aq)^((-)) rarrCH_3OH_(aq)+Br_(aq)^-`, the rate law is: `rate = k[CH_3Br][OH^-]`.
How does reaction rate changes if `[OH^-]` is decreased by a factor of 5?

From the reaction: CH_3Br(aq) +OH_(aq)^((-)) rarr CH_3OH_(aq)+Br_(aq)^- , the rate law is: rate = k[CH_3Br][OH^-] . What is change in rate if concentrations of both reactants are doubled?

Following reaction: (CH_(3))_(3)C-Br +H_(2)O rarr (CH_(3))_(3)C-OH +HBr is an example of -

For the rection 2NOBr(g) rarr 2NO_2(g)+Br(g) , the rate law is rate = k[NOBr]^2 . If the rate of reaction is 6.5x10^(-6)mole L^(-1) s the concentration of NOBr is 2xx10^(-3) mole L^(-1) . What be the rate constant for the reaction?

The rate law for the reaction C_2H_4Br_2+3I^- rarr C_2H_4+2Br^-+I_3^- is rate = k[C_2H_4Br_2] [I^-] . The rate of the reaction is found to be 1.1xx10^(-4)M//s when the concentrations of C_2H_4Br_2 and I^- are 0.12M and 0.18M respectively. Calculate the rate constant of the reaction.

Consider the reaction :- Tl^+(aq)+2Ce^(4+)(aq) rarr Tl^(3+)(aq) + 2Ce^(3+)(aq) The rate law for the reaction is as rate = k [Ce^(4+)] [Mn^(2+)] . In the presence of Mn^(2+) the reaction occurs in the following elementary steps: a) Ce^(4+)(aq) + Mn^(2+)(aq) rarr Ce^(3+)(aq)+ Mn^(3+)(aq) , b) Ce^(4+) (aq) + Mn^(3+)(aq)rarrCe^(3+)(aq) +Mn^(4+)(aq) ,c) Tl^+ (aq) +, Mn^(3+)(aq)rarr Tl^(3+)(aq) + Mn^(2+)(aq) :-Identify :- intermediate

Consider the reaction :- Tl^+(aq)+2Ce^(4+)(aq) rarr Tl^(3+)(aq) + 2Ce^(3+)(aq) The rate law for the reaction is as rate = k [Ce^(4+)] [Mn^(2+)] . In the presence of Mn^(2+) the reaction occurs in the following elementary steps: a) Ce^(4+)(aq) + Mn^(2+)(aq) rarr Ce^(3+)(aq)+ Mn^(3+)(aq) ,b) Ce^(4+) (aq) + Mn^(3+)(aq)rarrCe^(3+)(aq) +Mn^(4+)(aq), c) Tl^+ (aq) +, Mn^(3+)(aq)rarr Tl^(3+)(aq) + Mn^(2+)(aq) Identify:-catalyst

For the reaction, 3I^(o-)(aq) + S_2O_8^(2(o-))(aq)rarr I_3^(o-) (aq) + 2 SO_4^(2(o-))(aq) Calculate the rate of formation of I_3^(o-) , the rates of consumption of I^- and S_2O_8^(2(o-)) and' the overall rate of reaction if the rate of formation of SO_4^(2(o-)) is 0.022M/s

Consider the reaction : CH_(3)CH_(2)CH_(2)Br+NaCN to CH_(3)CH_(2)CH_(2)CN+NaBr This reaction will be the fastest in

Write the rate law for the following reactions:- A reaction that is second order in NO and first order in Br_2

The rate law for the reaction RCl + NaOH(aq) rarr ROH + NaCl is given by Rate = k[RCl] . The rate of the reaction will be