In the balanced equation for combustion of 1 mole of butane, $C_{4} H_{10} (g)$ , the coefficient of oxygen is:

5/2

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9/2

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13/2

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Solution

The correct option is D 13/2
Balanced chemical reaction of butane:
$C_{4} H_{10} + \frac{13}{2} O_{2} \to 4 C O_{2} + 5 H_{2} O$

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Similar questions

During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is
(a) $2 C_{4} H_{10} (g) + 13 O_{2} (g) \to 8 C O_{2} (g) + 10 H_{2} O (l); Δ_{c} H = - 2658.0 k J m o l^{- 1}$
(b) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = - 1329.0 k J m o l^{- 1}$
(c) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = - 2658.0 k J m o l^{- 1}$
(d) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = + 2658.0 k J m o l^{- 1}$

Q. The ratio of number of moles of butane to the number of moles of oxygen necessary for complete combustion of butane is:

Q. Can you write the balanced chemical equation for the combustion of the fuel butane

(C_{4} H_{10})

C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) ⟶ 4 C O_{2} (g) + 5 H_{2} O (l); Δ H = - 2878 k J

Δ H

is the heat of combustion of butane gas.If true enter 1 else 0

Q. What is the sum of the coefficients in the balanced equation for the complete combustion of 2-methylbutane? Use smallest whole number coefficients. Do not forget coefficients of 1.

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In the balanced equation for combustion of 1 mole of butane, C4H10(g), the coefficient of oxygen is:

The correct option is D 13/2Balanced chemical reaction of butane:C4H10+132O2→4CO2+5H2O

In the balanced equation for combustion of 1 mole of butane, $C_{4} H_{10} (g)$ , the coefficient of oxygen is:

The correct option is D 13/2
Balanced chemical reaction of butane:
$C_{4} H_{10} + \frac{13}{2} O_{2} \to 4 C O_{2} + 5 H_{2} O$