Combustion of ethane gas is an exothermic reaction. Which of the following best describes the temperature conditions that are likely to make the combustion of ethane gas a spontaneous change? (4 points) Any temperature, because combustion of ethane leads to an increase in entropy. Any temperature, because combustion of ethane leads to a decrease in entropy. Low temperature only, because combustion of ethane leads to an increase in entropy. High temperature only, because combustion of ethane leads to a decrease in entropy.

Any temperature, because combustion of ethane leads to an increase in entropy.  

Explanation:

2C₂H₆(g) + 7O₂(g) ⟶ 4CO₂(g) + 6H₂O(g); ΔH <0

Δn(gas) = 10 - 9. so

ΔS > 0

The requirement for spontaneity is that

ΔG = ΔH - TΔS < 0

ΔH is negative.

ΔS positive, so TΔS is positive.

ΔG = (a negative term) - (a positive term) = a negative term

ΔG is always negative, so the reaction is always spontaneous.

B is wrong, because ΔS is positive.

C and D are wrong, because the reaction is always spontaneous.

hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)