(D) Given: $P_1 = 3 \, atm$,$T_1 = -23 \, ^oC = (-23 + 273) \, K = 250 \, K$. At $Place \, B$,$T_2 = 30 \, ^oC = (30 + 273) \, K = 303 \, K$. Accordin

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(D) Given: $P_1 = 3 \, atm$,$T_1 = -23 \, ^oC = (-23 + 273) \, K = 250 \, K$. At $Place \, B$,$T_2 = 30 \, ^oC = (30 + 273) \, K = 303 \, K$. According to Gay-Lussac's Law,for a fixed amount of gas at constant volume,$\frac{P_1}{T_1} = \frac{P_2}{T_2}$. Substituting the values: $\frac{3}{250} = \frac{P_2}{303}$. $P_2 = \frac{3 \times 303}{250} = \frac{909}{250} = 3.636 \, atm \approx 3.64 \, atm$.

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

Medium

$A$ truck carrying an oxygen cylinder is coming from $Place \, A$. At $Place \, A$,the gas in the cylinder is at a temperature of $-23 \, ^oC$ and a pressure of $3 \, atm$. When the truck passes through $Place \, B$,the temperature is $30 \, ^oC$. What will be the pressure of the oxygen gas in $atm$?

A
$2.64$
B
$1.64$
C
$1$
D
$3.64$

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Class 11

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States of Matter

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Ideal gas equation and Related gas laws

At $300 \ K$ temperature,the pressure of $2.5 \ g$ of $N_2$ gas is $4 \ bar$ and its volume is $2.5 \ L$. If the pressure becomes $10 \ bar$ at the same temperature,calculate its new volume. (in $L$)

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Pure hydrogen sulphide is stored in a tank of $100 \, L$ capacity at $20 \, ^oC$ and $2 \, atm$ pressure. The mass of the gas will be ............... $g$.

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At $17\,^{\circ}C$ temperature,the volume of a gas is $400\, mL$. At what temperature will: $(i)$ the volume become double,and $(ii)$ the volume become half?

Medium

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Densities of a gas at different conditions are in the ratio $1:2$ and their temperatures are in the ratio $2:1$,then the ratio of their respective pressure is :-

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At $0\,^{\circ}C$ temperature and $1\, atm$ pressure,the volume of a gas is $100\, cc$. If the pressure is increased by $1.5$ times and the temperature is increased by one-third of its absolute temperature,what will be the final volume of the gas in $cc$?

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At $300 \ K$ temperature,the pressure of $2.5 \ g$ of $N_2$ gas is $4 \ bar$ and its volume is $2.5 \ L$. If the pressure becomes $10 \ bar$ at the same temperature,calculate its new volume. (in $L$)

Pure hydrogen sulphide is stored in a tank of $100 \, L$ capacity at $20 \, ^oC$ and $2 \, atm$ pressure. The mass of the gas will be ............... $g$.

At $17\,^{\circ}C$ temperature,the volume of a gas is $400\, mL$. At what temperature will: $(i)$ the volume become double,and $(ii)$ the volume become half?

Densities of a gas at different conditions are in the ratio $1:2$ and their temperatures are in the ratio $2:1$,then the ratio of their respective pressure is :-

At $0\,^{\circ}C$ temperature and $1\, atm$ pressure,the volume of a gas is $100\, cc$. If the pressure is increased by $1.5$ times and the temperature is increased by one-third of its absolute temperature,what will be the final volume of the gas in $cc$?

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