Advertisements
Advertisements
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 ______.
पर्याय
3A → 2B + C
2B → 3A + C
2B + C → 3A
3A + 2B → C
Advertisements
उत्तर
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 2B + C → 3A.
APPEARS IN
संबंधित प्रश्न
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 \[\ce{A + 2B -> C}\], the instantaneous rate of reaction at a given instant can be represented by ____________.
In a reaction \[\ce{2A + P -> A2P}\], the reactant 'A' disappears at ____________.
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.
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 ______.
What is the relation between `("d"["H"_2])/"dt" and ("d"["NH"_3])/"dt"`?
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?
What is the rate of formation of ‘C’ in the following reaction?
A + 2B → 2C
