When carbon and oxygen combine in a combustion reaction, 394 kJ of energy are released for each mole of carbon dioxide that is produced. Compare this amount with the energy released in our sun when 1 mole of helium-4 is produced from 4 protons. $$\begin{array} { l l }
\text { helium- } 4 \text { mass } & 4.002602 \mathrm {~g} / \mathrm { mol } \
\text { ( } 2 \text { protons, } 2 \text { neutrons, } 2 \text { electrons) } & \
\text { proton mass } & 1.007279 \mathrm {~g} / \mathrm { mol } \
\text { neutron mass } & 1.008665 \mathrm {~g} / \mathrm { mol } \
\text { electron mass } & 5.485799 \times 10 ^ { - 4 } \mathrm {~g} / \mathrm { mol } \
\text { speed of light } & 2.997924 \times 10 ^ { 8 } \mathrm {~m} / \mathrm { s }
\end{array}$$

Question

When carbon and oxygen combine in a combustion reaction, 394 kJ of energy are released for each mole of carbon dioxide that is produced. Compare this amount with the energy released in our sun when 1 mole of helium-4 is produced from 4 protons. $$\begin{array} { l l } 
\text { helium- } 4 \text { mass } & 4.002602 \mathrm {~g} / \mathrm { mol } \
\text { ( } 2 \text { protons, } 2 \text { neutrons, } 2 \text { electrons) } & \
\text { proton mass } & 1.007279 \mathrm {~g} / \mathrm { mol } \
\text { neutron mass } & 1.008665 \mathrm {~g} / \mathrm { mol } \
\text { electron mass } & 5.485799 \times 10 ^ { - 4 } \mathrm {~g} / \mathrm { mol } \
\text { speed of light } & 2.997924 \times 10 ^ { 8 } \mathrm {~m} / \mathrm { s }
\end{array}$$

Quizplus · Accepted Answer

The Answer of When carbon and oxygen combine in a combustion reaction, 394 kJ of energy are released for each mole of carbon dioxide that is produced. Compare this amount with the energy released in our sun when 1 mole of helium-4 is produced from 4 protons. $$\begin{array} { l l } 
\text { helium- } 4 \text { mass } & 4.002602 \mathrm {~g} / \mathrm { mol } \
\text { ( } 2 \text { protons, } 2 \text { neutrons, } 2 \text { electrons) } & \
\text { proton mass } & 1.007279 \mathrm {~g} / \mathrm { mol } \
\text { neutron mass } & 1.008665 \mathrm {~g} / \mathrm { mol } \
\text { electron mass } & 5.485799 \times 10 ^ { - 4 } \mathrm {~g} / \mathrm { mol } \
\text { speed of light } & 2.997924 \times 10 ^ { 8 } \mathrm {~m} / \mathrm { s }
\end{array}$$

When Carbon and Oxygen Combine in a Combustion Reaction, 394