From the equation $C + 2 H_{2} {S O}_{4} \to {C O}_{2} + {2 H}_{2} O + 2 {S O}_{2}$ . Calculate the mass of the carbon oxidized by 49g of sulphuric acid. (Atomic mass of C=12, H=1, S=32, O=16)

4 g

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3 g

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6 g

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Solution

The correct option is D 3 g
$C + 2 H_{2} {S O}_{4} ⟶ {C O}_{2} + 2 H_{2} O + 2 {S O}_{2}$
$49 g$ of $H_{2} {S O}_{4}$
Molar Mass of $H_{2} {S O}_{4}$ = ${98 g m o l}^{- 1}$
$N o . o f m o l e s = \frac{G i v e n M a s s}{M o l a r M a s s} = \frac{49}{98} = \frac{1}{2} 2 m o l e s o f H_{2} {S O}_{4} ⟶ 1 m o l e o f C 1 m o l e o f H_{2} {S O}_{4} ⟶ \frac{1}{2} m o l e o f C \frac{1}{2} m o l o f \frac{1}{2} m o l e = \frac{1}{2} \times \frac{1}{2} m o l e o f C = \frac{1}{4} m o l e o f C \frac{1}{4} m o l e o f C M o l e = \frac{G i v e n M a s s}{A t o m i c M a s s} \frac{1}{4} = \frac{x}{12} \frac{12}{4} = x 3 = x$
Mass of Carbon oxidized by $49 g$ of $H_{2} {S O}_{4}$ is $3 g$

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Similar questions

From the equation:

C + 2H₂SO₄ → CO₂+ 2H₂O +2SO₂

Calculate:

The mass of carbon oxidized by 49 g of sulphuric acid (C = 12; relative molecular mass of sulphuric acid = 98).

C + 2 H_{2} S O_{4} ⟶ C O_{2} + 2 H_{2} O + 2 S O_{2}

Calculate the mass of carbon oxidized by 49 gm of sulphuric acid.

(a) from the equation"
$C + 2 H_{2} S O_{4} \to C O_{2} + 2 H_{2} O + 2 S O_{2}$
Calculate:
(i) hte mass of carbon oxidized by 49 g of sulphuric acid.
(ii) the volume of sulphur dioxide measured at STP, linerated at the same time.
(b) (i) A compound has the following percentage composition by mass; carbon 14.4 % hydrogen 1.2% and chlorine 84.5 % . Determine the empirical formula of this compound. Work correct to 1 decimal place. (H - 1; C = 12; Cl = 35.5)
(ii) The relativ molecular mass of this compound is 168, so what is its molecular formuka?