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Standard XII

Physics

For the react...

Question

For the reaction
$2 X (g) \to 2 Y (g) + 2 Z (g)$
Time in min.
0
100
200
The partial pressure of X in mm of Hg
800
400
200
Assuming ideal gas nature,
calculate, the order of reaction:

1st order

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2nd order

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zero order

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None of these

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Solution

The correct option is A 1st order
$2 X (g) \to 2 Y (g) + 2 Z (g)$
Time in minutes $0$ $100$ $200$
Partial pressure
of X in mm of Hg $200$ $800$ $400$

From the given data, it can be seen that along with time, the partial pressure of X decreases linearly and so, the rate law is $r = k [X]$ and the order of reaction is one.

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Similar questions

Observation No.	Time (in minute)	$P_{x}$ (in mm of Hg)
1	0	800
2	100	400
3	200	200

At constant temperature and volume

X

decomposes as

2 X (g) \to 3 Y (g) + 2 Z (g)

, where

P_{x}

is the partial pressure of

X

. What is the order of reaction with respect to

X

?
(i) Find the rate constant.
(ii) Find the time for 75% completion of the reaction.
(iii) Find total pressure when pressure of

X

is 700 mm of Hg.

Q. A constant temperature and volume

X

decomposes as,

2 X (g) ⟶ 3 Y (g) + 2 Z (g)

P_{X}

is the partial pressure of

X

Observation No.	Time $(m i n)$	$P_{X} (i n m m H g)$
$1$	$0$	$800$
$2$	$100$	$400$
$3$	$200$	$200$

(i)

What is the order of the reaction with respect to

X

(i i)

Find the rate constant.

(i i i)

Find the time for

75

% completion of the reaction.

(i v)

Find the total pressure when pressure of

X

700

m m

H g

Q. For the first order gaseous reaction,

x (g) \to 2 y (g) + z (g)

, the initial pressure,

P_{x} = 90

mm Hg. The pressure after 10 minutes is 180 mm Hg. The rate constant of the reaction is:

Observation no.	Time (in min)	$P_{x} (i n m m H g)$
1	0	800
2	100	400
3	200	200

At constant temperature and volume, $X$ decomposes according to first order kinetics as follows:
$2 X (g) \to 3 Y (g) + 2 Z (g)$
where $P_{x}$ is the partial pressure of $X$ .

Which of the following statements is true for the given reaction?

Observation no.	Time (in min)	$P_{x} (i n m m H g)$
1	0	800
2	100	400
3	200	200

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Time in min.	0	100	200
The partial pressure of X in mm of Hg	800	400	200

For the reaction2X(g)→2Y(g)+2Z(g)Time in min.0100200The partial pressure of X in mm of Hg800400200Assuming ideal gas nature, calculate, the order of reaction:

The correct option is A 1st order 2X(g)→2Y(g)+2Z(g)Time in minutes 0 100 200Partial pressure of X in mm of Hg 200 800 400From the given data, it can be seen that along with time, the partial pressure of X decreases linearly and so, the rate law is r=k[X] and the order of reaction is one.

For the reaction
$2 X (g) \to 2 Y (g) + 2 Z (g)$
Time in min.
0
100
200
The partial pressure of X in mm of Hg
800
400
200
Assuming ideal gas nature,
calculate, the order of reaction: