$A$ balloon contains $2.27 \ L$ of air and has a pressure of $1.013 \times 10^5 \ Nm^{-2}$. The balloon rises to a certain height and expands to a volume of $4540 \ mL$. What is the final pressure of air in the balloon?
- A$2.026 \times 10^2 \ Nm^{-2}$
- B$5.065 \times 10^4 \ Nm^{-2}$
- C$4.540 \times 10^4 \ Nm^{-2}$
- D$5.065 \times 10^{-4} \ Nm^{-2}$
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Similar Questions
Pressure of $1 \, g$ of an ideal gas $A$ at $27^{\circ} C$ is found to be $2 \, bar$. When $2 \, g$ of another ideal gas $B$ is introduced in the same flask at the same temperature,the pressure becomes $3 \, bar$. Find a relationship between their molecular masses.
Medium
View Solution$A$ certain mass of gas occupies a volume of $300 \, cc$ at $27 \, ^oC$ and $620 \, mm$ pressure. The volume of this gas at $47 \, ^oC$ and $640 \, mm$ pressure will be ........... $cc$.
Medium
View SolutionAt $27^{\circ} C$,$1 \ L$ of $H_2$ with a pressure of $1 \ bar$ is mixed with $2 \ L$ of $O_2$ with a pressure of $2 \ bar$ in a $10 \ L$ flask. What is the pressure exerted by the gaseous mixture in $bar$? (Assume $H_2$ and $O_2$ as ideal gases)
At what temperature in $K$ will $28 \ g$ of $N_2$ gas occupy a volume of $10.0 \ L$ at $2.46 \ atm$ pressure?
Medium
View SolutionMatch the laws given in List-$I$ with their mathematical forms given in List-$II$.
List-$I$ List-$II$ $(1)$ Boyle's Law $(A)$ $p \propto T$ $(2)$ Charles's Law $(B)$ $V \propto n$ $(3)$ Gay-Lussac's Law $(C)$ $p \propto \frac{1}{V}$ $(4)$ Avogadro's Law $(D)$ $pV = nRT$ $(5)$ Ideal Gas Equation $(E)$ $V = k_2T$
| List-$I$ | List-$II$ |
| $(1)$ Boyle's Law | $(A)$ $p \propto T$ |
| $(2)$ Charles's Law | $(B)$ $V \propto n$ |
| $(3)$ Gay-Lussac's Law | $(C)$ $p \propto \frac{1}{V}$ |
| $(4)$ Avogadro's Law | $(D)$ $pV = nRT$ |
| $(5)$ Ideal Gas Equation | $(E)$ $V = k_2T$ |
Medium
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