(A) Given:$T_1 = 75^{\circ}C = 348 \, K$$V_1 = V$$V_2 = V - 0.15V = 0.85V$$P_1 = P$$P_2 = 2P$Using the combined gas law: $\frac{P_1 V_1}{T_1} = \frac{

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(A) Given:$T_1 = 75^{\circ}C = 348 \, K$$V_1 = V$$V_2 = V - 0.15V = 0.85V$$P_1 = P$$P_2 = 2P$Using the combined gas law: $\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$Substituting the values:$\frac{P \times V}{348} = \frac{2P \times 0.85V}{T_2}$$\frac{1}{348} = \frac{1.7}{T_2}$$T_2 = 348 \times 1.7 = 591.6 \, K$Converting to Celsius:$T_2(^{\circ}C) = 591.6 - 273.15 = 318.45^{\circ}C \approx 319^{\circ}C$

Class 11 Chemistry States of Matter Ideal gas equation and Related gas laws

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If a sample of neon gas at $75^{\circ}C$ is cooled such that its volume decreases by $15\%$,to what temperature (in $^{\circ}C$) should it be heated so that its pressure becomes double?

A
$319$
B
$592$
C
$128$
D
$60$

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Class 11

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States of Matter

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Ideal gas equation and Related gas laws

$A$ $2.24\,L$ oxygen cylinder shows a leakage at $NTP$. When the leakage is plugged,the pressure drops by $570\,mm\,Hg$. What is the number of moles of gas that escaped?

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$A$ flask of $1 \ L$ capacity is heated from $25 \ ^oC$ to $35 \ ^oC$. What volume of air (in $mL$) will be expelled from the flask?

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The variation of volume of an ideal gas with its number of moles $(n)$ is obtained as a graph at $300 \ K$ and $1 \ atm$ pressure. What is the slope of the graph?

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The following $P$ vs $V$ curve is plotted. What is the relation between $T_1$,$T_2$ and $T_3$?

Medium

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What will be the volume in $L$ of $2.8 \ g$ of carbon monoxide at $27 \ ^oC$ temperature and $0.821 \ atm$ pressure? $(R = 0.0821 \ L \ atm \ mol^{-1} K^{-1})$

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If a sample of neon gas at $75^{\circ}C$ is cooled such that its volume decreases by $15\%$,to what temperature (in $^{\circ}C$) should it be heated so that its pressure becomes double?

Similar Questions

$A$ $2.24\,L$ oxygen cylinder shows a leakage at $NTP$. When the leakage is plugged,the pressure drops by $570\,mm\,Hg$. What is the number of moles of gas that escaped?

$A$ flask of $1 \ L$ capacity is heated from $25 \ ^oC$ to $35 \ ^oC$. What volume of air (in $mL$) will be expelled from the flask?

The variation of volume of an ideal gas with its number of moles $(n)$ is obtained as a graph at $300 \ K$ and $1 \ atm$ pressure. What is the slope of the graph?

The following $P$ vs $V$ curve is plotted. What is the relation between $T_1$,$T_2$ and $T_3$?

What will be the volume in $L$ of $2.8 \ g$ of carbon monoxide at $27 \ ^oC$ temperature and $0.821 \ atm$ pressure? $(R = 0.0821 \ L \ atm \ mol^{-1} K^{-1})$

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