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What would happen to the rate of a reaction with rate law rate k (NO2) (H2) if the concentration of Anna were doubled?
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What would happen to the rate of a reaction if the concentration of substrate was increased after the point of saturation?
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What would happen to the rate of a reaction with rate law rate k NO H2 if the concentrations of NO were doubled?
The rate would be four times larger
What would happen to the rate of a reaction with rate law rate kNO2H2 if the concentration of NO were double?
The rate would quadruple (increase by a factor of 4). This is because the rate depends on the SQUARE of the concentration of NO.
What would happen to the rate of a reaction with law rate k NO2H2 if the concentration of H2 were halved?
The rate would be four times larger. Impossible.
What would happen to the rate of a reaction with rate law rate equals k NO 2 H2 if the concentration of NO were halved?
It will decrease by half.
What would happen to the rate of a reaction with rate law kNO2H2 if the concentration of NO were doubled?
The rate would be four times larger
What would happen to the rate of a reaction with rate law rate kno2h2 if the no were doubled?
the rate would be four times larger. apex
What would happen to the rate of a reaction if the concentration of substrate was increased after the point of saturation?
zff
What would happen to the rate of a reaction with rate law rate k NO H2 if the concentrations of NO were doubled?
The rate would be four times larger
What would happen to the rate of a reaction with rate law rate k NO2H2 if the concentration of NO were doubled?
The rate would be one-fourth. Correct on Apex.
What would happen to the rate of a reaction with rate law rate kNO2H2 if the concentration of NO were double?
The rate would quadruple (increase by a factor of 4). This is because the rate depends on the SQUARE of the concentration of NO.
What would happen to the rate of a reaction with rate law rate k NO 2 H2 if the concentration of NO were halved?
The reaction rate would decrease
What would happen to the rate of a reaction with rate law rate k NO 2 H2 if the concentration of H2 were halved?
The rate would also behalved
What would happen to the rate of a reaction with law rate k NO2H2 if the concentration of H2 were halved?
The rate would be four times larger. Impossible.
What would happen to the rate of a reaction with rate law rate equals k NO 2 H2 if the concentration of NO were halved?
It will decrease by half.
What would happen to the rate of a reaction with rate law rate k no 2 h2 if the concentration of h2 were halved-?
This rate law suggests its rate to be direct proportional to H2 concentration, thus halving this would implicate a halved reaction rate.
How is rate of a chemical reaction usually expressed?
Rates of reaction can be expressed depending upon their order.For example say you have a reaction between two chemicals and the initial rate for that reaction is known :-when:-The concentration of one of the reactants is doubled and the other reactants concentration remains the same and the overall rate of reaction does not change - reaction is zero orderwith respect to chemical which was doubled.The concentration of one of the reactants is doubled and other reactants concentration remains the same and the overall rate of reaction doubles - reaction is first order with respect to chemical which was doubled.The concentration of one of the reactants is doubled and other reactants concentration remains the same and the overall rate of reaction quadruples - reaction is second order with respect to chemical which was doubled.Zero Orderrate = kFirst Orderrate = k [A] (reaction is 1st order with respect to [A] and 1st order overall)Second Orderrate = k [A][B] (reaction is first order with respect to [A] and first order with respect to[B], reaction is second order overall)rate = k [A]2 (reaction is second order with respect to [A] and second order overall)Orders are simply added together in order to determine the overall order of reaction :-rate = k [A][B][C] would be third order overall and first order with respect to each of the reactantsThere are other orders of reaction, for example 2 and 3 quarter orders and third order reactions, but these are a little more complex.
