Question

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?

Answer #1

Molar mass of C6H6,

MM = 6*MM(C) + 6*MM(H)

= 6*12.01 + 6*1.008

= 78.108 g/mol

mass(C6H6)= 7.700 g

use:

number of mol of C6H6,

n = mass of C6H6/molar mass of C6H6

=(7.7 g)/(78.11 g/mol)

= 9.858*10^-2 mol

Since Δ H is negative, heat is released

when 2 mol of C6H6 reacts, heat released = 6542.0 KJ

So,

for 9.858*10^-2 mol of C6H6, heat released = 9.858*10^-2*6542.0/2 KJ

= 3.225*10^2 KJ

This heat is absorbed by water

Given:

Q = 322500 J

m = 5691 g

C = 4.184 J/g.oC

Ti = 21 oC

use:

Q = m*C*(Tf-Ti)

322500 = 5691.0*4.184*(Tf-21.0)

Tf -21.0 = 13.5 oC

Tf = 34.5 oC

Answer: 34.5 oC

The following equation is the balanced combustion reaction for
C6H6:
2C6H6(l) + 15O2(g) ------>
12CO2(g)+6H2O(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

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)

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When one mole of C6H6 is burned, 3.27 MJ of heat is produced.
When the heat from burning 7.19 g of C6H6 is added to 5.69 kg of
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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
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Express your answer to four significant figures and include the
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ΔG∘ =
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Thermochemical Equations 07a (kJ)
Consider the following thermochemical equation for the
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Calculate the heat associated with the consumption of 1.158 mol
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Use the correct sign for q
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Part C
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