1)Which of the following is true? a)As a reaction at constant temperature and pr
ID: 822122 • Letter: 1
Question
1)Which of the following is true?
a)As a reaction at constant temperature and pressure goes to equilibrium, |?G| decreases.
b)The standard state for solutes is the pure solute at 1 atm.
c)The larger ?G°, the faster the reaction.
d)When a reaction reaches equilibrium, ?G° = 0.
2)At 25°C, ?G°f is -620 kJ/mol for SiCl4(g) and -592 kJ/mol for MgCl2(s). Calculate ?G° for the reaction, SiCl4(g) + 2 Mg(s) ? 2 MgCl2(s) + Si(s) and determine if the reaction is spontaneous at 25°C if the pressure of SiCl4(g) is 1 atm.
a)?G° = 28 kJ; the process is nonspontaneous.
b)?G° = -564 kJ; the process is nonspontaneous.
c)?G° = 28 kJ; the process is spontaneous.
d)?G° = -564 kJ; the process is spontaneous.
3)If Q increases
a)?G decreases and the reaction becomes less spontaneous.
b)?G increases and the reaction becomes less spontaneous.
c)?G increases and the reaction becomes more spontaneous.
d)?G decreases and the reaction becomes more spontaneous
Explanation / Answer
1) d)When a reaction reaches equilibrium, ?G° = 0.
2)
delta G = 2 x -592 - (-620) = -564 KJ/mol
d)?G° = -564 kJ; the process is spontaneous.
3) d)?G decreases and the reaction becomes more spontaneous since delta G = -RT ln Q
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