Reaction is producing more reactants than products
The enthalpy of combustion of 1 mole of benzene is 3169 kJ/mol .
The first step in answering this question is to obtain the balanced thermochemical equation of the reaction. The thermochemical equation shows the amount of heat lost or gained.
The thermochemical equation for the combustion of benzene is;
2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔrH° = -3169 kJ/mol
We can see that 1 mole of benzene releases about 3169 kJ/mol of heat.
Learn more: brainly.com/question/13164491
SI unit of frequency is Hertz(Hz)
Answer:
Explanation:
We want the energy required for the transition:
CO 2
(
s
)
+
Δ
→
C
O
2
(
g
)
Explanation:
We assume that the temperature of the gas and the solid are EQUAL.
And thus we simply have to work out the product:
2
×
10^
3
⋅
g
×
196.3
⋅
J
⋅
g
−
1 to get an answer in Joules as required.
What would be the energy change for the reverse transition:
C
O
2
(
g
)
+
→
C
O
2
(
s
)
?
