Question

The following equation is the balanced combustion reaction for C6H6:

2C_{6}H_{6}(l) + 15O_{2}(g) ------>
12CO_{2}(g)+6H_{2}O(l)+6542 kJ

If 6.900 g of C6H6 is burned and the heat produced from the burning is added to 5691 g of water at 21 °C, what is the final temperature of the water?

please answer this is due today thank you

Answer #1

2C6H6(l) + 15O2(g) -------> 12CO2(g) + 6H2O(l) + 6542kJ

So, 6542 KJ of heat is relesed by two mole of C6H6 Combustion

Therefore,

Heat released per 1 mole of combustion of C6H6 = 3271kJ = 3271000J

Mass of C6H6 = 6.900g

Molar mass of C6H6 = 78.11g/mol

No of mole of C6H6 = 6.900g/78.11(g/mol)=0.08834

Therefore,

Heat released by 0.08834 mole of C6H6 burning = 0.08834 × 3271000J = 288960J

Heat released by reaction = Heat absorbed by water

q=m × ∆T × C

where,

q = Heat absorbed by water,

m = mass of water ,5691g

∆T = Temperature raise

C = heat capacity of water , 4.184J/g ℃

Therefore,

288960J = 5691g × ∆T × 4.184J/g ℃

∆T = 12.14℃

Initial temperature =21℃

Therefore,

Final temperature = 21℃ + 12.14℃ = 33.14℃

The balanced combustion reaction for C6H6 is
2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ If 7.700 g C6H6 is burned
and the heat produced from the burning is added to 5691 g of water
at 21 ∘ C, what is the final temperature of the water?

The following equation is the balanced combustion reaction for
C6H6:
2C6H6(l)+15O2(g) = 12CO2(g)+6H2O(l)+6542KJ
If 7.800 g of C6H6 is burned and the heat produced from the
burning is added to 5691 g of water at 21 °C, what is the final
temperature of the water?

The following equation is the balanced combustion reaction for
C6H6:
2C6H6 (l) + 15O2 (g) --> 12CO2(g) + 6H2O(l)+6542KJ
If 8.800 g of C6H6 is burned and the heat produced from the
burning is added to 5691 g of water at 21 Celcius, what is the
final temp of the water? (in celcius)

If 5.000 g of C6H6 is burned and the heat produced from the
burning is added to 5691 g of water at 21 °C, what is the final
temperature of the water?

What mass of oxygen is needed for the complete combustion of 122
mL of
C6H6 (molar mass = 78.1 g/mol) to
produce carbon dioxide and water?
Density of C6H6 = 0.88 g/mL
2C6H6(l) +
15O2(g)
12CO2(g) +
6H2O(l)

Estimate the carbon-carbon bond strength in benzene given:
2C6H6(g)+15O2(g)⟶12CO2(g)+6H2O(g) ΔH∘=−6339kJ
Bond dissociation data are the following: the strength of the O=O
bond in O2 is 498 kJ/mol, the strength of the C=O bond in CO2 is
804 kJ/mol, the strength of the H−O bond in H2O is 460 kJ/mol, the
strength of the H−C bond in benzene is 410 kJ/mol.

Part A
Write an equation for the combustion of one mole of benzene,
C6H6(g).
Express your answer as a chemical equation. Identify all of the
phases in your answer.
2C6H6(g)+15O2(g)→12CO2(g)+6H2O(l)
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Correct
Part B
Determine ΔG∘ at 298 K if the products of the combustion
are CO2(g) and H2O(l) . (ΔG∘ f(C6H6(g))= 129.8
kJmol−1, ΔG∘ f(CO2(g))=-394.4 kJmol−1 ,
ΔG∘f(H2O(l))= -237.1 kJmol−1).
Express your answer to four significant figures and include the
appropriate units.
ΔG∘ =
-3208 kJ
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Use the correct sign for q
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