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).

8 g

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4 g

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6 g

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5 g

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3 g

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Solution

The correct option is E
3 g

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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.

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)

(a) (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 relative molecular mass of this compound is 168, so what is its molecular formula?
(iii) By what type of reaction could this compound be obtained from ethyne?

(b) From the equation:
C + 2H₂SO₄ $\overset{}{\to}$ CO₂ + 2H₂O + 2SO₂
Calculate:
(i) the mass of carbon oxidised by 49 g of sulphuric acid (C = 12; relative molecular mass of sulphuric acid = 98).
(ii) the volume of sulphur dioxide measured at STP, liberated at the same time.
(Volume occupied by 1 mole of a gas at STP is 22.4 dm³).

(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?

From the equation.:

C + 2H₂SO₄ → CO₂+ 2H₂O +2SO₂

Calculate:

The volume of sulphur dioxide measured at STP, liberated at the same time.

(Volume occupied by 1 mole of a gas at STP is 224 dm³)

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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).

The correct option is E 3 g

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).

The correct option is E
3 g