Following mechanism has been proposed for a reaction,
2A+B D+E
A+B C+D ...(Slow)
A+ C E ...(Fast)
The rate law expression for the reaction is:
1. r = K[A]2[B]
2. r=K[A][B]
3. r= K[A]2
4. r= K[A][C]
For the reaction N2 + 3H2 2NH3, the rate = 2 x 10-4 M s-1 .Therefore, the rate is given as:
1. 10-4 Ms-1
2. 104 Ms-1
3. 10-2 sM-1
4. 10-4 sM-1
When ethyl acetate was hydrolysed in pressure of 0.1 N HCl, the rate constant was found to be 5.40 x 10-5 sec-1 . But when 0.1 N H2SO4 was used for hydrolysis, the rate constant was found to be 6.25 X10-5sec-1. Thus, it may be concluded that:
1. H2SO4 is stronger than HCI
2. H2SO4 is weaker than HCl
3. H2SO4 and HCl both have the same strength
4. The data are not sufficient to compare the strength of H2SO4 and HCI
The chemical reaction, 2O3 3O2 proceeds as follows;
O3 O2 + O .....(Fast)
O+O3 2O2 ....(Slow)
The rate law expression should be:
1. r = K[O3]2
2. r = K[O3]2[O2]-1
3. r = K[O3][O2]
4. unpredictable
The rate of reaction becomes 2 times for every 10°C rise in temperature. How the rate of reaction will increase when temperature is increased from 30°C to 80°C?
1. 16
2. 32
3. 64
4. 128