According to the equation C6 H6(1)+(15)/(2) O2( g) →6 CO2( g)+3 H2 O(l), Δ/ /=-3264.4 kJ / mol,

step 1 According to equation, benzene reacts with 15 over 2 molecule of oxygen in gaseous state to form

According to the equation C6 H6(1)+(15)/(2) O2( g) →6...

According to the equation $\mathrm{C}_{6} \mathrm{H}_{6}(1)+\frac{15}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow$ $6 \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}), \Delta / /=-3264.4 \mathrm{~kJ} / \mathrm{mol}$, the energy evolved when $7.8 \mathrm{~g}$ of benzene is burnt in air will be (1) $163.32 \mathrm{~kJ} / \mathrm{mol}$ (2) $326.4 \mathrm{~kJ} / \mathrm{mol}$ (3) $32.64 \mathrm{~kJ} / \mathrm{mol}$ (4) $3.264 \mathrm{~kJ} / \mathrm{mol}$

According to the equation $\mathrm{C}_{6} \mathrm{H}_{6}(1)+\frac{15}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow$
$6 \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}), \Delta / /=-3264.4 \mathrm{~kJ} / \mathrm{mol}$, the energy
evolved when $7.8 \mathrm{~g}$ of benzene is burnt in air will be
(1) $163.32 \mathrm{~kJ} / \mathrm{mol}$
(2) $326.4 \mathrm{~kJ} / \mathrm{mol}$
(3) $32.64 \mathrm{~kJ} / \mathrm{mol}$
(4) $3.264 \mathrm{~kJ} / \mathrm{mol}$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Enthalpy of Reaction

This concept refers to the energy change that accompanies a chemical reaction, typically measured in kilojoules (kJ). In exothermic reactions, like combustion, energy is released as the reaction proceeds. Understanding how to use the given enthalpy change per mole allows one to calculate the total energy released for any given amount of reactant by scaling it appropriately.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to quantify the relationships between the amounts in moles of reactants and products. It provides the framework for converting between mass and moles, which is crucial when determining how much energy is released based on the number of moles of a substance involved in the reaction.

Mole Concept and Molar Mass

The mole concept is central to chemistry and allows quantitative conversion between the mass of a substance and the number of particles present using its molar mass. It is essential for determining how many moles are present in a given mass of a substance, enabling proper calculations of energy changes when combined with stoichiometric relationships.

Transcript

Please give Ace some feedback