Question

Butane combusts in the atmosphere and releases heat:2C4H10(g) + 13 O2(g) ---> 8 CO2(g) + 10 H2O(g)The signs of the values for ΔG, ΔH, and ΔS for this reaction would be+, +, -+, -, --, -, +-, +, +

Answer 1

Answer:
`\Delta G`: -ve

`\Delta H` : -ve,

`\Delta S` : +ve

Step-by-step explanation:

Endothermic reactions are those in which heat is absorbed by the system and exothermic reactions are those in which heat is released by the system.

`\Delta H` for Endothermic reaction is positive and
`\Delta H` for Exothermic reaction is negative.

Entropy is the measure of randomness or disorder of a system. If a system moves from an ordered arrangement to a disordered arrangement, the entropy is said to decrease and vice versa.

`\Delta S` is positive when randomness increases and
`\Delta S` is negative when randomness decreases.

`2C_4H_(10)(g)+13O_2(g)\rightarrow 8CO_2(g)+10H_2O(g)`

As 15 moles of gaseous reactants are changing into 18 moles of gaseous products, randomness is increasing and thus
`\Delta S` is positive.

Using Gibbs Helmholtz equation:

`\Delta G=\Delta H-T\Delta S`

`\Delta G=(-ve)-T(+ve)`

`\Delta G=(-ve)(-ve)=-ve`

Thus
`\Delta H` is negative ,
`\Delta S` is positive and
`\Delta G` is negative.