Advertisements
Advertisements
Question
Choose the most correct option.
The rate law for the reaction aA + bB → P is rate = k[A] [B]. The rate of reaction doubles if _________.
Options
concentrations of A and B are both doubled.
[A] is doubled and [B] is kept constant
[B] is doubled and [A] is halved
[A] is kept constant and [B] is halved.
Solution
The rate law for the reaction aA + bB → P is rate = k[A] [B]. The rate of reaction doubles if [A] is doubled and [B] is kept constant
APPEARS IN
RELATED QUESTIONS
Answer the following in brief.
How instantaneous rate of reaction is determined?
Rate constant for the reaction \[\ce{2N2O5 -> 4NO2 + O2}\] is 4.98 × 10–4 s–1. Find the order of reaction?
In a chemical reaction, \[\ce{2A + B -> C + D}\] Find the INCORRECT statement.
If concentration of reactant 'A' is increased by 10 times the rate of reaction becomes 100 times. What is the order of reaction, if rate law is, rate = k[A]x?
For the reaction \[\ce{H2_{(g)} + I2_{(g)} ⇌ 2HI_{(g)}}\], the average rate of reaction is expressed as ____________.
In a reaction \[\ce{2A + P -> A2P}\], the reactant 'A' disappears at ____________.
For the reaction \[\ce{N2 + 3H2 ⇌ 2NH3}\]; if `(∆["NH"_3])/(∆"t")` = 2 × 10−4 mol dm−3 s−1, the value of `(-Δ["N"_2])/(∆"t")` would be ____________.
Which of the following expressions is CORRECT for the rate of formation of Br2?
\[\ce{5Br^-_{( aq)} + BrO^-_{3(aq)} + 6H^+_{( aq)} -> 3Br2_{(aq)} + 3H2O_{(l)}}\]
What is the average rate of reaction when the change in concentration of product is 0.05 Min 20 seconds?
Average rate of reaction for the following reaction.
\[\ce{2SO2 (g) + O2(g) -> 2SO3 (g)}\] is written as ______.
For the reaction,
\[\ce{2NO(g) + O2(g) -> 2NO2(g) ->[d(NO2)][dt] = 0.052 mol dm^{-3} s^{-1}}\]
Calculate rate of consumption of NO (g).
What is the relation between `("d"["H"_2])/"dt" and ("d"["NH"_3])/"dt"`?
In the reaction A + 3B → 2C, the rate of formation of C is ______.
Define the rate of a reaction.
Explain the term instantaneous rate of a reaction.
Explain factors affecting the rate constant of a chemical reaction.
For the reaction, \[\ce{3I^-(aq) + S2O^2-_8(aq) -> I^-_3(aq) + 2SO^2-_4(aq)}\]
`(d[SO_4^(2-)])/dt = 2.2 xx 10^(-2)` M/s at a particular time.
Calculate `(a) -(d[I^-])/dt (b) -(d[S_2O_8^(2-)])/dt (c) (d[I_3^-])/dt`
What is the rate law for reaction
\[\ce{2NO_{2(g)}-> 2NO_{(g)} + O_{2(g)}}\]
