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 ______.
Answer the following in brief.
How instantaneous rate of reaction is determined?
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?
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?
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 ______.
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?
