Question

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)

Answer #1

The balanced combustion reaction for C_{6}H_{6}
is---

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

Now, C_{6}H_{6} =( 12 x 6 ) +(1 x 6) = 72 + 6 =
78 g

The above equation indicates that 2x78 = 156 g
C_{6}H_{6} will produce 6542 KJ

Now, by using proportions we can then calculate that ---

x/6542kJ = 8.800 g / 156g

=> x = 6542 x 8.800 g / 156 g

=> x =57569.6 /156 KJ

=> x = 369.035 KJ

=> x = 369035 J (heat)

We have the relation,

heat(Q) = mass(m) *specific heat(c) * T

=>T = 369035 J / (5691g x 4.18J/g°C)

=> T=
15.5^{0}C

**Therefore, final temperature = (21 + 15.5)° C=
36.5°C**

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)+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 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?

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)

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
SubmitMy...

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
water at 21.0°C, what is the final temperature of the water?

Thermochemical Equations 07a (kJ)
Consider the following thermochemical equation for the
combustion of butane.
2C4H10(g)+15O2(g)→8CO2(g)+10H2O(g)ΔH∘rxn=−5314.6kJ
Part A
Calculate the heat associated with the consumption of 1.158 mol
of O2 in this reaction.
Use the correct sign for q
q =
+
kJ
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Incorrect; Try Again; 6 attempts remaining
Part B
Calculate the heat associated with combustion of 29.46 g of
butane.
Use the correct sign for q
q =
kJ
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Part C
Calculate the...

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.

1. 3.000 grams of Ca is burned in a bomb calorimeter. The
water’s temperature rose from 20.0 degrees centigrade to 21.79
degrees centigrade. The heat capacity of the calorimeter is 26.60
kJ/C. What is the enthalpy change for this reaction as written. The
thermochemical equation is:
2Ca (s) + O2 (g) —> 2CaO (s)
2. 1.30 grams of C7H6O2 is combusted in a bomb calorimeter.
The water’s temperature rose from 20.00 degrees centigrade to 21.58
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