Question

37. Considering the reaction
C(s) +1/202(g)—>CO(g) + 200 kJ
The signs of AH, AS and AG respectively are
(1) +,-,-
(2) -, +, +
(3)-,-,-
(4) -, +, -
please give full explanation​

Answer 1

Explanation:

Notice that the standard enthalpy change of reaction,

Δ

H

∘

, is given to you in kilojoules per mole, which means that it corresponds to the formation of one mole of carbon dioxide.

C

(s]

+

O

2(g]

→

CO

2(g]

More specifically, when one mole of carbon reacts with one mole of oxygen gas, one mole of carbon dioxide is produced and

393 kJ

of heat are given off.

Remember, a negative enthalpy change of reaction tells you that heat is being given off, i.e. the reaction is exothermic.

Now, in order to determine how much carbon is needed in order for the reaction to give off

275 kJ of heat , use the fact that one mole of carbon is needed to give off

393 kJ

of hea

275

kJ

⋅

1 mole C

393

kJ

=

0.6997 moles C

To see how many grams of carbon would contain this many moles, use carbon's molar mass

0.6997

moles C

⋅

12.011 g

1

mole C

=

8.40 g

So, when

8.40

grams of carbon react with enough oxygen gas, the reaction will give off

275 kJ

of heat. This is equivalent to having a standard enthalpy change of reaction equal to

Δ

H

∘

=

−

275 kJ

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