Question

Calculate the heat associated with the consumption of 1.542 mol of O2 in this reaction.

Calculate the heat associated with combustion of 25.08 g of butane.

Calculate the mass of butane that must be burned in order to
heat 23.83 kg of water from 22.31 ∘*C* to 65.71 ∘C. Assume
no loss of heat in the transfer from the reaction to the water. The
specific heat of water is 4.184 J/g∘C.

Consider the following thermochemical equation for the
combustion of butane.

2C4H10(*g*)+15O2(*g*)→8CO2(*g*)+10H2O(*g*)Δ*H*∘rxn=−5314.6kJ

Answer #1

**2C4H10(g)+15O2(g) → 8CO2(g)+10H2O(g) ΔH∘rxn =
−5314.6kJ**

**a) 15 mol O2 = -5314.6 kj**

**so that,**

**1.542 mol O2 on consumption = -5314*1.542/15 = -546.3
kj**

**b)**

**No of mol of butane = 25.08 / 58 = 0.432
mol**

**so that**

**amount of energy released = 0.432*5314/2 = 1147.824
kj**

**c)**

**heat absorbed by water = m*s*DT**

** = 23.83*10^3
*4.18*(65.71-22.31)**

** = 4323.05 kj**

**2 mol butane = - 5314.6 kj**

**No of mol of butane = 4323.05*2/5314 = 1.63
mol**

**mass of butane = 1.63*58 = 94.54 grams**

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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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...

2C4H10(g)+13 O2(g)--> 10H2O(g)+8CO2(g)
A. calculate the mass of water produced when 6.30g of
butane (C4H10) reacts with excess oxygen.
B. calculate the mass of butane needed to produce
47.2g of carbon dioxide

Consider, for example, the reaction
2NO(g)+O2(g)⇌2NO2(g)
Then the standard heat of reaction for the overall reaction
is
ΔH∘rxn=ΔH∘f(products)−−ΔH∘f(reactants)
ΔH∘rxn=2(33.2)-[2(90.2)+0]= -114kJ
Part A
For which of the following reactions is ΔH∘rxn equal to
ΔH∘f of the product(s)?
You do not need to look up any values to answer this
question.
Check all that apply.
Na(s)+12Cl2(l)→NaCl(s)
2Na(s)+Cl2(g)→2NaCl(s)
Na(s)+12Cl2(g)→NaCl(s)
H2(g)+12O2(g)→H2O(g)
2H2(g)+O2(g)→2H2O(g)
H2O2(g)→12O2(g)+H2O(g)
Part B
The combustion of heptane, C7H16, occurs via the reaction
C7H16(g)+11O2(g)→7CO2(g)+8H2O(g)
with heat of formation values given by the following...

Question 4
Part A
Using the following equation for the combustion of octane,
calculate the heat of reaction for 100.0 g of octane. The molar
mass of octane is 114.33 g/mole.
2 C8H18 + 25 O2 → 16
CO2 + 18 H2O ΔH°rxn = -11018
kJ
Using the following equation for the combustion of octane,
calculate the heat of reaction for 100.0 g of octane. The molar
mass of octane is 114.33 g/mole.
2 C8H18 + 25 O2 → 16...

18. Butane gas burns according to the following exothermic
reaction:
C4H10 (g) + 13/2 O2 (g) → 4 CO2 (g) + 5 H2O (g) ∆H°rxn = -
2877.1 kJ
a) If 25.0 g of butane were burned, how much energy would be
released?
b) If the reaction of 25.0 g of butane produced a volume change
of 15.4 L against an external pressure of 748 mmHg, calculate the
work done (in J).
c) Calculate the change in internal energy (∆E)...

Calculate heat of combustion reaction of 1.0 g of octane:
2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O
The calorimeter contains 1200 g water, and the temperature
changes from 25.00 deg C to 33.20 deg C. Heat capacity of bomb is
837 J/deg C.

Use Hess's Law to calculate the enthalpy of reaction, ΔH rxn,
for the reaction in bold below given the following chemical steps
and their respective enthalpy changes. Show ALL work!
2 C(s) + H2(g) → C2H2(g) ΔH°rxn = ?
1. C2H2(g) + 5/2 O2(g) → 2CO2 (g) + H2O (l) ΔH°rxn = -1299.6
kJ
2. C(s) + O2(g) → CO2 (g) ΔH°rxn = -393.5 kJ
3. H2(g) + ½ O2(g) → H2O (l) ΔH°rxn = -285.8 kJ

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
degrees centigrade. The heat capacity...

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?

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