Browse by Stream
QnA
Home
QnA
Go To Your Study Dashboard

Get Answers to all your Questions

header-bg qa

1 mole of \mathrm{H}_2 gas is contained in a box of volume V=100 \mathrm{~cm}^3 at T=300 \mathrm{~K}. The gas is heated to a temperate of T=3000 \mathrm{~K} and the gas converted to a gas of hydrogen atoms. The final pressure would be - 

Option: 1

Same as the pressure initially


Option: 2

2 times the pressure initially


Option: 3

10 times the preesure initially


Option: 4

20 times the preesure initially


Answers (1)

best_answer

Consider the diagram, when the molecules breaks into atoms, the number of moles, would become twice.

PV=nRT

As volume (V) of the containers are constant

As gases break number of moles becomes twice of initial.

So, n_2=2n,

\begin{aligned} & \Rightarrow P_{\propto n T} \\ & \begin{aligned} \Rightarrow \frac{P_2}{P_1}=\frac{n_2 T_2}{n_1 T_1} & =\frac{2 n_1 \times 3000}{n_1 \times 300} \\ & =20 \end{aligned} \end{aligned}

P_2=20 P_1

Hence, final pressure ofthe gas would be 20 times the pressure initially.

Posted by

Rakesh

View full answer

NEET 2024 Most scoring concepts

    Just Study 32% of the NEET syllabus and Score up to 100% marks

Similar Questions

Trending Articles/News

anam-khan

Re-NEET UG 2026: Education minister seeks cooperation of states, UTs for fair and smooth conduct of exam
anam-khan

Tamil Nadu NEET UG Cut-offs: Madras Medical College, CMC Vellore among top choices
anam-khan

NEET Paper Leak Case: Delhi court sends Pune physics lecturer to six-day CBI custody

Latest Question