Question
Calculate the heat of reaction in kcal at 25 °C and 1 atm for the following...
Calculate the heat of reaction in kcal at 25 °C and 1 atm for the following reaction per mol from the given data in the table below. C3H8 (l) + O2 (g) à CO2 (g) + H2O (l) Compound DHo f (kcal/mol) DHv at 25 °C (kcal/mol) C3H8 (g) 24.820 3.823 CO2 (g) 94.052 1.263 H2O (g) 57.798 10.519 Hint: pay attention to phases!
Homework Answers
Answer #1
The standard heat of reaction is given by the following equation:
The balanced chemical equation is given by:
The governing equation gets reduced to:
Given that:
ΔHH2O(l)o = ΔHH2O(g)o + ΔHH2Ov = - 57.798 + (- 10.519) = - 68.317 kcal/mol
ΔHCO2(g)o = - 94.052 kcal/mol
ΔHC3H8(l)o = ΔHC3H8(g)o + ΔHC3H8v = - 24.82 + (- 3.823) = - 28.643 kcal/mol
ΔHO2(g)o = 0 (By definition)
Sustituting these values in the governing equation.
ΔHoreaction = (3 X (- 94.052) + 4 X (- 68.317) - (-28.643) - 5 X 0)
ΔHoreaction = - 282.156 - 273.268 + 28.643
ΔHoreaction = -526.781 kcal / mol
which is the required standard heat of reaction.
Not the answer you're looking for?
Similar Questions
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g)...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm
and 25 °C:
C2H6 (g) + O2 (g) →
CO2 (g) + H2O (l) (unbalanced)
ΔHf C2H6 (g) = -84.7 kJ/mol; S
C2H6 (g) = 229.5 J/K⋅mol;
ΔHf ∘ CO2 (g) = -393.5 kJ/mol; S
CO2 (g) = 213.6 J/K⋅mol;
ΔHf H2O (l) = -285.8 kJ/mol; SH2O
(l) = 69.9 J/K⋅mol;
SO2 (g) = 205.0 J/K⋅mol
Use the following calorimetric data to calculate the heat of combustion (burning) of the carbon compound...
Use the following calorimetric data to calculate the heat of
combustion (burning) of the carbon compound shown below:
C3H8 (g) + 5O2 (g) →
3CO2(g) + 4H2O(g)
reaction
ΔHo (kJ)
C(s) + O2(g) → CO2(g)
-393.5
C(s) → C(g)
+718.4
H2O(l) → H2O(g)
+44.0
H2(g) + 1/2 O2(g) →
H2O(l)
-285.8
3C(s) + 4H2(g) → C3H8(g)
-103.8
C(s) + 2H2(g) + 1/2O2(g) →
CH3OH(l)
-238.7
6C(s) + 3H2(g) → C6H6(g)
+82.9
C6H6(l) →
C6H6(g)
+33.9
CH3OH(l) → CH3OH(g)
+38.0
ΔHo...
1- Calculate ΔG o for the following reaction at 25°C. You will have to look up...
1- Calculate ΔG o for the following reaction at 25°C.
You will have to look up the thermodynamic data. 2 C2H6(g) + 7
O2(g) → 4 CO2(g) + 6 H2O(l)
2- A reaction will be spontaneous only at low
temperatures if both ΔH and ΔS are negative. For
a reaction in which ΔH = −320.1 kJ/mol and ΔS =
−99.00 J/K ·mol,determine the temperature (in °C)below which the
reaction is spontaneous.
Use the table to calculate delta G rxn for the following reaction at 25 degree C....
Use the table to calculate delta G rxn for the following
reaction at 25 degree C.
A.) 2Mg(s) +O2(g) --> 2MgO(s)
B.) 2SO2(g) +O2(g) --> 2SO3(g)
C.) 2C2H2(g) + 5O2(g) --> 4CO2(g) + 2H2O(l)
Species
Delta G (kJ/mol)
Mg(s) 0
O2
(g) 0
MgO(s) -255.0
SO2(g)
-300.57
SO3(g)
-370.53
C2H2(g)
168.43
CO2(g)
-394.65
H2O(l)
-237.35
H2O(g)
-228.77
Find the ΔH and ΔE for the reaction below: C2H6(g) + 7/2 O2(g) à 2 CO2(g)...
Find the ΔH and ΔE for the reaction below:
C2H6(g) + 7/2 O2(g) à 2
CO2(g) + 3 H2O (l)
given the following data:
ΔHf C2H6 = -84.7
kJ/mol
ΔHf CO2 = -393.5 kJ/mol
ΔHf H2O = -286 kJ/mol
Given the following information below, use Hess’s Law to calculate the enthalpy of formation for sodium...
Given the following information below, use Hess’s Law to
calculate the enthalpy of formation for sodium oxide:
Na (s) +
HCl (l) à NaCl (aq) + ½ H2
(g)
∆HRx
= -393.1 kJ/mol
Na2O (s)
+ 2 HCl (l) à 2 NaCl
(aq) + H2O
∆HRx
= -675.2 kJ/mol
H2 (g)
+ ½ O2
(g) à H2O
(g) ∆HRx
= -288.1 kJ/mol
2 Na (s)
+ ½ O2
(g) à Na2O
(s)
∆HRx
= __________ kJ/mol
Calculated Heat of Reaction is....?
(Put your answer in...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...
The standard heat of formation, ΔH∘f, is defined as the
enthalpy change for the formation of one mole of substance from its
constituent elements in their standard states. Thus, elements in
their standard states have ΔH∘f=0. Heat of formation
values can be used to calculate the enthalpy change of any
reaction.
Consider, for example, the reaction
2NO(g)+O2(g)⇌2NO2(g)
with heat of formation values given by the following table:
Substance
ΔH∘f
(kJ/mol)
NO(g)
90.2
O2(g)
0
NO2(g)
33.2
Then the heat of...
For the reaction: 2 C (s) + H2(g) →C2H2(g) a) Calculate the enthalp
For the reaction:
2 C (s) + H2(g) →C2H2(g)
a) Calculate the enthalpy of reaction (DHrxn) from the following
reactions:
Reaction
Δ
Hrxn(kJ/mol)2
C2H2(g)+ 5 O2(g) → 4 CO2(g) + 2 H2O
(l)
-2599.2
C (s) + O2(g) →
CO2(g)
-
393.5
2 H2(g) + O2(g) → 2H2O
(l)
-571.8
b) If the DS for the reaction is equal to 652 J/mol, and the
reaction proceeds at 25°C, would you expect the reaction to be
spontaneous?
solve question 2 based on the result of question 1 Question 1 Acetone (C3H6O (l)) burns...
solve question 2 based on the result of question 1
Question 1
Acetone (C3H6O (l)) burns in oxygen according to the
equation:
4 O2(g) +
C3H6O(l) = 3
CO2(g) + 3H2O(l
At 25 °C the enthalpy change for this reaction is -1789.9 kJ.
The standard enthalpy of formation ∆fHo of
CO2 (g) and H2O (l) are -393.5 1 and -285.83
kJ/mol, respectively. Determine the enthalpy of formation of
C3H6O(l) at 25 °C. Please enter your
answer (unit: kJ/mol) with...
When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00 atm, H2O (l)...
When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00
atm, H2O (l) and CO2 (g) are formed with the evolution of 50.33 kJ
of energy.
Substance
∆Hºf (kJ mol -1)
Sº (J mol -1 K -1)
H2O (l)
- 285.8
69.95
CO2 (g)
- 393.5
213.7
O2 (g)
0.0
205.0
C3H8 (g)
?
270.2
Calculate the molar enthalpy of combustion, ∆Hºcomb , of propane
and the standard molar enthalpy of formation, ∆Hºf , of propane
gas.
ADVERTISEMENT
Need Online Homework Help?
Get Answers For Free
Most questions answered within 1 hours.
ADVERTISEMENT
Active Questions
asked 13 minutes ago
asked 13 minutes ago
asked 45 minutes ago
asked 49 minutes ago
asked 53 minutes ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 2 hours ago