A gaseous reaction A(g)↔2B(g)+C(g) is found to be of first order. If the reaction is started with pA=90 mm Hg, the total pressure after 10min is found to be 180 mm Hg. The rate constant of the reaction is

1.  4.60x10-3s-1

2.  6.9x10-2s-1

3.  1.15x10-3s-1

4.  4.90x10-3s-1

View Answer  
4
Correct Answer :

1.15x10-3s-1


Explanation :
No Explanation available for this question

The rate of the reaction: 2SO2+O2↔2SO3 may be expressed as: -d[O2]/dt=2.5x10-4mol L-1 sec-1 The rate of reaction when expressed in terms of SO3 will be

1.  -5.0x10-4mol L-1 sec-1

2.  -1.25x10-4mol L-1 sec-1

3.  3.75x10-4mol L-1 sec-1

4.  5.0x10-4mol L-1 sec-1

View Answer  
4
Correct Answer :

5.0x10-4mol L-1 sec-1


Explanation :
No Explanation available for this question

The rate determining step in a reaction is A + 2B -> C. Doubling the concentration of B would make the reaction to proceed:

1.  At the same rate

2.  Twice more rapidly

3.  Four times more fast

4.  Four times more slow

View Answer  
4
Correct Answer :

Four times more fast


Explanation :
No Explanation available for this question

For a first order reaction: R→ Pt1/2 is proportional to

1.  [A]1/2

2.  [A]0

3.  [A]

4.  1/[A]

View Answer  
4
Correct Answer :

[A]0


Explanation :
No Explanation available for this question

For a chemical reaction, A+B→C,it has been found that: (i) rate becomes double when the conc. of A is doubled (ii) rate becomes 16 times when the concentration of both A and B are doubled. The rate expression is:

1.  Rate =k[A]2[B]

2.  Rate =k[A][B]3

3.  Rate =k[A]2[B]3

4.  Rate =k[A]2

View Answer  
4
Correct Answer :

Rate =k[A][B]3


Explanation :
No Explanation available for this question

For the reaction, 2A+B+C→A2B+C the rate law has been found to be Rate =k[A][B]2with [A]=0.1 mol L-1[B]=0.2mol L-1and [C]=0.8 mol L-1 is:

1.  6.4x10-8mol L-1s-1

2.  4x10-3mol L-1s-1

3.  8.0x10-9mol L-1s-1

4.  4.0x10-7mol L-1s-1

View Answer  
4
Correct Answer :

8.0x10-9mol L-1s-1


Explanation :
No Explanation available for this question

The half life period of a reaction is 100 min. In 400 min the initial concentration of 2.0 g will become

1.  0.25 g

2.  0.75 g

3.  0.125 g

4.  d.0.1 g

View Answer  
4
Correct Answer :

0.125 g


Explanation :
No Explanation available for this question

For a first order reaction, the time of a certain percentage change in reactant concentration will be proportional to

1.  time-1

2.  Initial conc. of reactant

3.  k1

4.  k1-1

View Answer  
4
Correct Answer :

k1-1


Explanation :
No Explanation available for this question

The specific rate constant for a first order reaction depends on the

1.  Concentration of the reactant

2.  Concentration of the product

3.  Time

4.  Temperature

View Answer  
4
Correct Answer :

Temperature


Explanation :
No Explanation available for this question

The rate for a first order reaction is 0.693x10-2mol dm-3min-1 and the initial concentration is 0.2mol dm3. The half life period is

1.  1200 s

2.  0.33 s

3.  20 s

4.  600 s

View Answer  
4
Correct Answer :

1200 s


Explanation :
No Explanation available for this question
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