(B) The combustion reaction for methane is as follows:$CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$Initial moles:$CH_4 = 10, O_2 = 50, CO_2 = 0, H_2O = 0$Sin

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(B) The combustion reaction for methane is as follows:$CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$Initial moles:$CH_4 = 10, O_2 = 50, CO_2 = 0, H_2O = 0$Since $CH_4$ is the limiting reagent, it will be completely consumed.For $10 \ \text{moles}$ of $CH_4$, $2 \times 10 = 20 \ \text{moles}$ of $O_2$ are consumed.Final moles:$O_2 = 50 - 20 = 30 \ \text{moles}$$CO_2 = 10 \ \text{moles}$$H_2O = 2 \times 10 = 20 \ \text{moles}$Thus, the number of moles of $O_2$, $H_2O$, and $CO_2$ are $30, 20, 10$ respectively.Option $B$ is the correct answer.

Class 11 Chemistry Some Basic Concepts of Chemistry Chemical equation and limiting reagent

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In a $1 \ L$ vessel, $10 \ \text{moles}$ of methane and $50 \ \text{moles}$ of $O_2$ are present. The number of moles of $O_2$, water, and $CO_2$ present in the vessel after the vessel is heated to burn methane completely are respectively:

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A
$30, 20, 20$
B
$30, 20, 10$
C
$20, 30, 10$
D
$20, 10, 30$

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Some Basic Concepts of Chemistry

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Chemical equation and limiting reagent

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$50.0 \, kg$ of $N_2 \, (g)$ and $10.0 \, kg$ of $H_2 \, (g)$ are mixed to produce $NH_3 \, (g)$. Calculate the amount of $NH_3 \, (g)$ formed. Identify the limiting reagent in the production of $NH_3$ in this situation.

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In a $1 \ L$ vessel, $10 \ \text{moles}$ of methane and $50 \ \text{moles}$ of $O_2$ are present. The number of moles of $O_2$, water, and $CO_2$ present in the vessel after the vessel is heated to burn methane completely are respectively:

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What is the value of $PV$ type of work for the following reaction at $1 \ bar$ pressure (in $J$)? The reaction is: $C_2H_4(g) + HCl(g) \rightarrow C_2H_5Cl(g)$. Given volumes are $200 \ mL$ of $C_2H_4$ and $150 \ mL$ of $HCl$.

For the reaction $2Al + 3MnO \xrightarrow{\Delta} Al_2O_3 + 3Mn$; If $108 \ g$ of $Al$ and $213 \ g$ of $MnO$ are heated,then which of the following is incorrect?

$50.0 \, kg$ of $N_2 \, (g)$ and $10.0 \, kg$ of $H_2 \, (g)$ are mixed to produce $NH_3 \, (g)$. Calculate the amount of $NH_3 \, (g)$ formed. Identify the limiting reagent in the production of $NH_3$ in this situation.

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