Chemistry, asked by gugan64, 5 months ago

 \sf \red{ \underline{question \ \: : }}
A sample of oxygen occupies 47.2 liters under a pressure of 1240 torr at 25°C. What volume would it occupy at 25°C if the pressure were decreased to
730 torr?

(a) 27.8 L
(b) 29.3 L
(c) 32.3 L
(d) 47.8 L

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Answers

Answered by BʀᴀɪɴʟʏAʙCᴅ
6

\huge\mathcal{\boxed{\fcolorbox{red}{aqua}{TO\:SEARCH;-}}} \\

  • The volume that would occupied at 25°C if the pressure were decreased to 730 torr .

\huge\mathcal{\boxed{\fcolorbox{red}{aqua}{SOLUTION;-}}} \\

CASE - 1 ;-

\begin{cases} {V_1 = 47.2 L} \\ {P_1 = 1240 torr = 1240 mm Hg} \\ {T_1 = 25^{\circ}C = 298 K} \end{cases} \\

CASE - 2 ;-

\begin{cases} {V_2 = ?} \\ {P_2 = 730 torr = 730 mm Hg} \\ {T_2 = 25^{\circ}C = 298 K} \end{cases} \\

✴️ We have know that,

\huge{\color{aqua}\star} \sf\purple{\dfrac{P_1\:V_1}{T_1}\:=\:\dfrac{P_2\:V_2}{T_2}\:} \\

\sf{\leadsto\:\dfrac{P_1\:V_1}{\cancel{T_1}}\:=\:\dfrac{P_2\:V_2}{\cancel{T_2}}\:} \\

\bf{\Big[\:\because\:T_1\:=\:T_2\:=\:25°\:\Big]} \\

\sf{\leadsto\:V_2\:=\:\dfrac{P_1\:V_1}{P_2}\:} \\

\sf{\leadsto\:V_2\:=\:\dfrac{1240\times{47.2}}{730}\:} \\

\sf{\leadsto\:V_2\:=\:\dfrac{58528}{730}\:} \\

\sf\green{\leadsto\:V_2\:=\:80.17\:L} \\

So, change in volume is,

\bf{V_2\:-\:V_1} \\

\bf{80.17\:-\:47.2} \\

\bf\red{32.97\:L\:\approx\:32.3\:L} \\

∴ (c) 32.3 L volume that the sample occupied at 25°C if the pressure were decreased to 730 torr .

Answered by Anonymous
3

Answer:

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