Consider the following chemical equation for the combustion of methane ( $C H_{4}$ )

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

Energy required to break bonds between C and H in $C H_{4}$ is more than the energy required to form them.

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Products have more energy than the reactants.

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Reactants have more energy than the products.

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Energy required to break bonds between C and H in $C H_{4}$ is less than the energy required to form them.

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Solution

The correct option is C
Reactants have more energy than the products.

The substances reacting are methane and oxygen (reactants). They have some amount of energy inside them. When they react, products (carbon dioxide and water) are formed which also have some energy in them. When the total energy of the reactants is more than total energy of the products. This difference of energy is released as heat of the reaction.

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Similar questions

Consider the following chemical equation for the combustion of methane ( $C H_{4}$ )

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

The heat of combustion of methane at 298 K is expressed by:

CH4(g)+2O2(g)→CO2(g)+2H2O(l);

ΔH=-890.2 KJ ΔE of the reaction at this temperature is?

Which one of the following chemical equations represent combustion reactions?

C + O_{2} \to C O_{2}

B: $C + \frac{1}{2} O_{2} \to C O$

C: $C O + \frac{1}{2} O_{2} \to C O_{2}$

Directions : The balanced chemical equation underneath each reaction description and answer the questions.

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

Methane burns readily in air.

Which type of flame is produced when ethane burns?

22 g C O_{2}

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

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