(D) The decomposition reaction is: $CH_3OH_{(g)} \to CO_{(g)} + 2H_{2(g)}$Initial moles: $CH_3OH = 0.01 \, mol$,$CO = 0$,$H_2 = 0$At equilibrium (comp

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(D) The decomposition reaction is: $CH_3OH_{(g)} \to CO_{(g)} + 2H_{2(g)}$Initial moles: $CH_3OH = 0.01 \, mol$,$CO = 0$,$H_2 = 0$At equilibrium (complete decomposition): $CH_3OH = 0 \, mol$,$CO = 0.01 \, mol$,$H_2 = 0.02 \, mol$Total moles of gas $n = 0.01 + 0.02 = 0.03 \, mol$Using the ideal gas law $PV = nRT$:$P = \frac{nRT}{V}$Given $R = 0.082 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$,$T = 600 \, K$,$V = 0.082 \, L$$P = \frac{0.03 \times 0.082 \times 600}{0.082}$$P = 0.03 \times 600 = 18 \, atm$

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

Medium

In a closed vessel of volume $0.082 \, dm^3$ at $600 \, K$,the complete decomposition of methanol vapor occurs as follows: $CH_3OH_{(g)} \to CO_{(g)} + 2H_{2(g)}$. If $0.01 \, mol$ of methanol is taken initially,what will be the pressure generated in the vessel in $atm$?

A
$3$
B
$6$
C
$12$
D
$18$

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Class 11

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States of Matter

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Ideal gas equation and Related gas laws

$2.9 \, g$ of a gas at $95^{\circ} C$ occupied the same volume as $0.184 \, g$ of dihydrogen at $17^{\circ} C$,at the same pressure. What is the molar mass of the gas?

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If $2$ moles of an ideal gas at $546 \ K$ has a volume of $44.8 \ L$,then what will be its pressure (in $atm$)? $(R=0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

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At $27\,^oC$ temperature,$4\,mol$ $Cl_2$,$4\,mol$ $N_2$,and $2\,mol$ $O_2$ are filled in a $5\,L$ closed vessel. Find the total pressure of the gaseous mixture. $(R = 8.34 \times 10^{-2} \,bar \,L \,mol^{-1} \,K^{-1})$ (in $,bar$)

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At a given temperature,the density of gas $x$ is twice the density of gas $y$. If the molar mass of $y$ is three times the molar mass of $x$,find the ratio of their pressures $(P_x/P_y)$.

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$300 \ mL$ of a gas at $27 \ ^\circ C$ is cooled to $-3 \ ^\circ C$ at constant pressure. The final volume is ................ $mL$.

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In a closed vessel of volume $0.082 \, dm^3$ at $600 \, K$,the complete decomposition of methanol vapor occurs as follows: $CH_3OH_{(g)} \to CO_{(g)} + 2H_{2(g)}$. If $0.01 \, mol$ of methanol is taken initially,what will be the pressure generated in the vessel in $atm$?

Similar Questions

$2.9 \, g$ of a gas at $95^{\circ} C$ occupied the same volume as $0.184 \, g$ of dihydrogen at $17^{\circ} C$,at the same pressure. What is the molar mass of the gas?

If $2$ moles of an ideal gas at $546 \ K$ has a volume of $44.8 \ L$,then what will be its pressure (in $atm$)? $(R=0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

At $27\,^oC$ temperature,$4\,mol$ $Cl_2$,$4\,mol$ $N_2$,and $2\,mol$ $O_2$ are filled in a $5\,L$ closed vessel. Find the total pressure of the gaseous mixture. $(R = 8.34 \times 10^{-2} \,bar \,L \,mol^{-1} \,K^{-1})$ (in $,bar$)

At a given temperature,the density of gas $x$ is twice the density of gas $y$. If the molar mass of $y$ is three times the molar mass of $x$,find the ratio of their pressures $(P_x/P_y)$.

$300 \ mL$ of a gas at $27 \ ^\circ C$ is cooled to $-3 \ ^\circ C$ at constant pressure. The final volume is ................ $mL$.

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