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Standard XII

Chemistry

Avogadro's Law & Gay Lussac's Law

Calculate the...

Question

Calculate the volume of oxygen required to burn completely a mixture of $22.4 d m^{3}$ of $C H_{4}$ and $11.2 d m^{3}$ of $H_{2}$ ?

50 d m^{3}

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52 d m^{3}

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50.4 d m^{3}

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51.4 d m^{3}

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Solution

The correct option is C $50.4 d m^{3}$
$C H_{4} + 2 O_{2} ⟶ C O_{2} + 2 H_{2} O$

$2 H_{2} + O_{2} ⟶ 2 H_{2} O$

$22.4 d m^{3} C H_{4}$ requires $2 \times 22.4 d m^{3} = 44.8 d m^{3} O_{2}$ .

$11.2 d m^{3} H_{2}$ requires $5.6 d m^{3} O_{2}$ .

$T o t a l v o l u m e = 50.4$ $d m^{3}$

Hence, the correct answer is option $C$ .

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Similar questions

Q. What volume of

O_{2}

is required to burn completely a mixture of

22.4 d m^{3}

C H_{4}

and

11.2 d m^{3}

H_{2}

?
The reactions are:

C H_{4} + 2 O_{2} \to C O_{2} + 2 H_{2} O

;

2 H_{2} + O_{2} \to 2 H_{2} O

(All volume at S.T.P).

What volume of oxygen is required to burn completely a mixture of $22.4 d m^{3}$ of methane and $11.2 d m^{3}$ of hydrogen into carbon dioxide and steam?
$C H_{4} + 20_{2} \to C O_{2} + 2 H_{2} O 2 H_{2} + O_{2} \to 2 H_{2} O$

What volume of oxygen is required to burn completely a mixture of 22.4 dm³ of methane and 11.2 dm³ of hydrogen into carbon dioxide and steam?

Equations of the reactions are given below. (Assume that all volumes are measured at STP).

CH₄ + 2O₂ → CO₂ +2H₂O

2H₂ + O₂ → 2H₂O

(a) What volume of oxygen is required to burn completely a mixture of 22.4 dm³of methane and 11.2 dm³ of hydrogen into carbon dioxide and steam? Equations of the reactions are given below:
CH₄ + 2O₂ $\overset{}{\to}$ CO₂ + 2H₂O
2H₂ + O₂ $\overset{}{\to}$ 2H₂O
(Assume that all volumes are measured at STP)

(b) The gases hydrogen, oxygen, carbon dioxide, sulphur dioxide and chlorine are arranged in order of their increasing relative molecular mass. Given 8 g of each gas at STP, which gas will contain the least number of molecules and which gas the most?

Q. The volume of oxygen at

S T P

required to burn

2.4 g

of carbon completely is:

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Calculate the volume of oxygen required to burn completely a mixture of 22.4 dm3 of CH4 and 11.2 dm3 of H2?

The correct option is C 50.4 dm3CH4+2O2⟶CO2+2H2O2H2+O2⟶2H2O22.4 dm3 CH4 requires 2×22.4 dm3=44.8 dm3 O2.11.2 dm3H2 requires 5.6 dm3 O2.Total volume=50.4 dm3Hence, the correct answer is option C.

Calculate the volume of oxygen required to burn completely a mixture of $22.4 d m^{3}$ of $C H_{4}$ and $11.2 d m^{3}$ of $H_{2}$ ?