(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

At $240.55 \ K$,for one mole of an ideal gas,a graph of $P$ (on $y$-axis) and $V^{-1}$ (on $x$-axis) gave a straight line passing through the origin. Its slope $(m)$ is $2000 \ J \ mol^{-1}$. What is the kinetic energy (in $J \ mol^{-1}$) of the ideal gas?

EasyAP EAMCET 2024

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At $400\, K$ temperature,the volume and pressure of a gas are $200\, mL$ and $1.5\, bar$ respectively. Calculate the volume,weight (assuming the gas is $N_2$),and the number of molecules at $STP$. $[R = 8.31 \times 10^{-2}\, L\, bar\, K^{-1}\, mol^{-1}]$.

Medium

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What will be the value of the gas constant $R$ when pressure is expressed in $dyne \, m^{-2}$ and volume in $mm^3$?

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On what factors do the values of the gas constant $R$ depend? What is its unit?

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$4 \ g$ of an ideal gas occupies $5.6035 \ L$ of volume at $546 \ K$ and $2 \ atm$ pressure. What is its molecular weight?

DifficultAP EAMCET 2002

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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

At $240.55 \ K$,for one mole of an ideal gas,a graph of $P$ (on $y$-axis) and $V^{-1}$ (on $x$-axis) gave a straight line passing through the origin. Its slope $(m)$ is $2000 \ J \ mol^{-1}$. What is the kinetic energy (in $J \ mol^{-1}$) of the ideal gas?

At $400\, K$ temperature,the volume and pressure of a gas are $200\, mL$ and $1.5\, bar$ respectively. Calculate the volume,weight (assuming the gas is $N_2$),and the number of molecules at $STP$. $[R = 8.31 \times 10^{-2}\, L\, bar\, K^{-1}\, mol^{-1}]$.

What will be the value of the gas constant $R$ when pressure is expressed in $dyne \, m^{-2}$ and volume in $mm^3$?

On what factors do the values of the gas constant $R$ depend? What is its unit?

$4 \ g$ of an ideal gas occupies $5.6035 \ L$ of volume at $546 \ K$ and $2 \ atm$ pressure. What is its molecular weight?

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