Advertisements
Advertisements
प्रश्न
Rate constant for the reaction \[\ce{2N2O5 -> 4NO2 + O2}\] is 4.98 × 10–4 s–1. Find the order of reaction?
Advertisements
उत्तर
Since the unit of rate constant is s–1, the reaction is first order.
APPEARS IN
संबंधित प्रश्न
The rate of reaction for certain reaction is expressed as:
`1/3(d[A])/dt=-1/2(d[B])/dt=-(d[C])/dt`
The reaction is ______.
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 _________.
Answer the following in brief.
How instantaneous rate of reaction is determined?
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 ____________.
For the reaction \[\ce{A + 2B -> C}\], the instantaneous rate of reaction at a given instant can be represented by ____________.
The rate of disappearance of SO2 in the reaction \[\ce{2SO2 + O2 -> 2SO3}\] is 1.28 × 10−3 mol dm−3 s−1. Then the rate of formation of SO3 is ____________ mol dm−3 s−1.
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 ____________.
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
\[\ce{2NO_{2(g)}-> 2NO_{(g)} + O_{2(g)}}\]
The rate constant for a first order reaction is 0.58 s-1 at 300 K and 0.026 s-1 at 290 K. What is the energy of activation? (R = 8.314 J K-1 mol-1)
Which of the following equations is correct regarding rate of disappearance of reactant and appearance of product for
N2(g) + 3H2(g) → 2NH3(g)
For the reaction, \[\mathrm{N_{2(g)}+3H_{2(g)}\longrightarrow2NH_{3(g)}}\]
N2(g) disappears at a rate of 2×10-4mol dm-3 s-1. Calculate rate of disappearance of H2?
