Question

Be sure to answer all parts. Be sure to report your answer to the correct number of significant figures. Calculate ΔG o and KP for the following processes at 25°C: (a) H2(g) + Br2(l) ⇌ 2HBr(g) ΔG o = kJ/mol KP = × 10 (Enter your answer in scientific notation.) (b) 1 2 H2(g) + 1 2 Br2(l) ⇌ HBr(g) ΔG o = kJ/mol KP = × 10 (Enter your answer in scientific notation.)

Answer 1

Answer: (a) The value of
`K_(p)` is
`4 * 10^(18)` and value of
`\Delta G^(o)` is -106.4 kJ/mol.

(b) The value of
`K_(p)` is
`2 * 10^(9)` and value of
`\Delta G^(o)` is -53.2 kJ/mol.

Step-by-step explanation:

(a) As the given reaction equation is as follows.

`H_(2)(g) + Br_(2)(l) \rightleftharpoons 2HBr(g)`

Firs, we will calculate the value of
`\Delta G^(o)` as follows.

`\Delta G^(o) = 2\Delta G^(o)_(F(HBr)) - \Delta G^(o)_{F(Br_(2))}`

=
`2 * -53.2 kJ/mol - (1) * (0) - (1) * (0)`

= -106.4 kJ/mol

`ln K_(p) = (-\Delta G^(o))/(RT)`

=
`(106.4 * 10^(3) J/mol)/(8.314 J/mol K * 298 K)`

`ln K_(p)` = 42.9

`K_(p) = 4 * 10^(18)`

Therefore, the value of
`K_(p)` is
`4 * 10^(18)` and value of
`\Delta G^(o)` is -106.4 kJ/mol.

(b) As the given reaction equation is as follows.

`(1)/(2)H_(2)(g) + (1)/(2)Br_(2)(l) \rightleftharpoons HBr(g)`

So,
`\Delta G^(o) = \Delta G^(o)_(F(HBr)) - (1)/(2)\Delta G^(o)_{F(Br_(2))}`

=
`(1)(-53.2 kJ/mol) - ((1)/(2))(0) - ((1)/(2))(0)`

= -53.2 kJ/mol

As,
`ln K_(p) = (-\Delta G^(o))/(RT)`

=
`(53.2 * 10^(3) J/mol)/(8.314 J/mol K * 298 K)`

= 21.5

`K_(p) = 2 * 10^(9)`

Therefore, the value of
`K_(p)` is
`2 * 10^(9)` and value of
`\Delta G^(o)` is -53.2 kJ/mol.