(B) The balanced chemical equation is: $2 Na(s) + 2 C_2H_5OH(\ell) \rightarrow 2 C_2H_5O^-Na^+ + H_2(g) \uparrow$ From the stoichiometry,$2 \times 23

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(B) The balanced chemical equation is: $2 Na(s) + 2 C_2H_5OH(\ell) \rightarrow 2 C_2H_5O^-Na^+ + H_2(g) \uparrow$ From the stoichiometry,$2 \times 23 \ g$ of $Na$ produces $1 \text{ mole}$ of $H_2$ gas. $46 \ g$ of $Na$ is equal to $2 \text{ moles}$ of $Na$. Since $2 \times 23 \ g$ $(46 \ g)$ of $Na$ produces $1 \text{ mole}$ of $H_2$,the amount of $H_2$ produced is $1 \text{ mole}$. Mass of $1 \text{ mole}$ of $H_2 = 2 \ g$. Converting to $kg$: $2 \ g = 2 \times 10^{-3} \ kg$.

Class 11 Chemistry Some Basic Concepts of Chemistry Chemical stoichiometry

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What is the quantity of hydrogen gas liberated when $46 \ g$ sodium reacts with excess ethanol? (Given Atomic mass of $Na = 23$)

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A
$2.4 \times 10^{-3} \ kg$
B
$2.0 \times 10^{-3} \ kg$
C
$4.0 \times 10^{-3} \ kg$
D
$2.4 \times 10^{-2} \ kg$

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Some Basic Concepts of Chemistry

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Chemical stoichiometry

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What is the quantity of hydrogen gas liberated when $46 \ g$ sodium reacts with excess ethanol? (Given Atomic mass of $Na = 23$)

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The volume of water to be added to $100 \, cm^3$ of $0.5 \, N \, H_2SO_4$ to get decinormal concentration is ........ $cm^3$.

When a $1.0 \, g$ mixture of $NaHCO_3$ and $Na_2CO_3$ is heated at $150^{\circ}C$,$112.0 \, mL$ of $CO_2$ is produced at $STP$. Calculate the percentage of $Na_2CO_3$ in the mixture. $(Na = 23, C = 12, O = 16)$

Three solutions of $HCl$ having normalities $12 \ N$,$6 \ N$,and $2 \ N$ are mixed to obtain a solution of $4 \ N$ normality. Which among the following volume ratios is incorrect for the above mixture?

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