The equation for the burning of octane is:

$2 C_{8} H_{18} + 25 O_{2} \to 16 C O_{2} + 18 H_{2} O$

If the relative molecular mass of carbon dioxide is 44.What is the mass of carbon dioxide produced by burning two moles of octane?

756 g

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700 g

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746 g

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704 g

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Solution

The correct option is D
704 g

$2 C_{8} H_{18} 2 m o l e s + 25 O_{2} \to 16 C O_{2} 16 m o l e s + 18 H_{2} O$

Mass of $C O_{2}$ = 16 $\times$ 44 = 704 g

By burning 2 moles of octane, 704 g of $C O_{2}$ is produced.

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Similar questions

The equation for the burning of octane is:
2C₈H₁₈ + 25O₂ $\overset{}{\to}$ 16CO₂ + 18H₂O
(i) How many moles of carbon dioxide are produced when one mole of octane burns?
(ii) What volume, at STP, is occupied by the number of moles determined in (i)?
(iii) If the relative molecular mass of carbon dioxide is 44, what is the mass of carbon dioxide produced by burning two moles of octane?
(iv) What is the empirical formula of octane?

The equation for the burning of octane is:

2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

How many moles of carbon dioxide are produced when one mole of octane burns?

The equation for the burning of octane is:

2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

What volume, at STP, is occupied by 8 moles of carbon dioxide ?

Q. The reaction of burning of carbon in oxygen is represented by the equation:

C_{(s)} + O_{2 (g)} \to {C O}_{2 (g)} + H e a t + L i g h t

When 9.0 g of solid carbon is burnt in 16.0 g of oxygen gas, 22.0 g of carbon dioxide is produced. The mass of carbon dioxide gas formed on burning of 3.0 g of carbon in 32.0 g of oxygen would be (Note : atomic mass of

C = 12.0 u, O = 16.0 u

4.5 moles of calcium carbonate are reacted with dilute hydrochloric acid.
(i) Write the equation for the reaction.
(ii) What is the mass of 4.5 moles of calcium carbonate? (Relative molecular mass of calcium carbonate is 100).
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The equation for the burning of octane is: 2C8H18+25O2→16CO2+18H2O If the relative molecular mass of carbon dioxide is 44.What is the mass of carbon dioxide produced by burning two moles of octane?

The correct option is D 704 g 2C8H182 moles+25O2→16CO216 moles+18H2O Mass of CO2​ = 16 × 44 = 704 g By burning 2 moles of octane, 704 g of CO2 is produced.

The equation for the burning of octane is:

$2 C_{8} H_{18} + 25 O_{2} \to 16 C O_{2} + 18 H_{2} O$

If the relative molecular mass of carbon dioxide is 44.What is the mass of carbon dioxide produced by burning two moles of octane?

The correct option is D
704 g

$2 C_{8} H_{18} 2 m o l e s + 25 O_{2} \to 16 C O_{2} 16 m o l e s + 18 H_{2} O$

Mass of $C O_{2}$ = 16 $\times$ 44 = 704 g

By burning 2 moles of octane, 704 g of $C O_{2}$ is produced.