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QUESTION
What volume of
CO_(2(g)) at STP is obtained by complete combustion of
6g carbon?
[2023]
(A)
22.4dm^(3)
(B)
11.2dm^(3)
◻
(C)
5.6dm^(3)
(D)
2.24dm^(3)

QUESTION $\newline$ What volume of $\text{CO}_{2(g)}$ at STP is obtained by complete combustion of $6\,\text{g}$ carbon? $\newline$ [ $2023$ ] $\newline$ (A) $22.4\,\text{dm}^{3}$ $\newline$ (B) $11.2\,\text{dm}^{3}$ $\newline$ (C) $5.6\,\text{dm}^{3}$ $\newline$ (D) $2.24\,\text{dm}^{3}$

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Find derivatives of sine and cosine functions

Full solution

Q. QUESTION

\newline

What volume of

\text{CO}_{2(g)}

at STP is obtained by complete combustion of

6\,\text{g}

carbon?

\newline

[

2023

]

\newline

(A)

22.4\,\text{dm}^{3}

\newline

(B)

11.2\,\text{dm}^{3}

\newline

(C)

5.6\,\text{dm}^{3}

\newline

(D)

2.24\,\text{dm}^{3}

Calculate moles of carbon: Calculate the moles of carbon used in the reaction. $\newline$ Molar mass of carbon (C) = $12 \, \text{g/mol}$ . $\newline$ Moles of carbon = mass / molar mass = $6 \, \text{g} / 12 \, \text{g/mol} = 0.5 \, \text{mol}$ .
Write chemical equation: Write the balanced chemical equation for the combustion of carbon. $\newline$ $\text{C(s)} + \text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)}.$ $\newline$ From the equation, $1$ mole of $\text{C}$ produces $1$ mole of $\text{CO}_2$ .
Calculate moles of CO $2$ : Calculate the moles of CO $2$ produced. $\newline$ Moles of CO $2$ = Moles of C = $0.5\,\text{mol}.$
Calculate volume at STP: Calculate the volume of CO $2$ at STP. $\newline$ At STP, $1$ mole of any gas occupies $22.4 \, \text{dm}^3$ . $\newline$ Volume of CO $2$ = Moles of CO $2$ $\times$ Volume per mole = $0.5 \, \text{mol} \times 22.4 \, \text{dm}^3/\text{mol} = 11.2 \, \text{dm}^3$ .

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