Question

(a) Consider the combustion of butane, given below: 2 C4H10(g) + 13 O2(g) 8 CO2(g) + 10 H2O(g) If C4H10(g) is decreasing at the rate of 0.850 mol/s, what are the rates of change of O2(g), CO2(g), and H2O(g)?

O2(g)/t = mol/s

CO2(g)/t = mol/s

H2O(g)/t = mol/s

(b) The decomposition reaction given below: 2 IF5(g) 1 I2(g) + 5 F2(g) is carried out in a closed reaction vessel. If the partial pressure of IF5(g) is decreasing at the rate of 470. torr/min, what is the rate of change of the total pressure in the vessel?

Ptot /t = torr/min

Answer #1

**a) rate of reaction = ( -1/2) d[C4H10]/[ dt = -( 1/13)
d[O2] / dt = ( 1/8) d[CO2] / dt = ( 1/10) d[H2O] / dt**

**given - d[C4H10] /dt = -0.85 mol/s**

**d[O2] /dt = ( 13/2) ( d[C4H10] / dt = -
5.525 mol/s ( -ve sign indicates decreasing
)**

**d[CO2] /dt = ( 8/2) (- d[C4H10] / dt = ( 4 x 0.85) =
3.4**

**d[H2O] /dt = (10/2) ( -d[C4H10] /dt = ( 10/2) x 0.85
=4.25**

**b) d [IF5] / dt = -0.47 torr /min**

**rate of rxn = - ( 1/2) d[IF5]/dt = d[I2] /dt = ( 1/5)
d[F2] / dt**

**d[O2] /dt = ( -1/2) ( -0.47) = 0.235
torr/min**

**d[F2] /dt = -( 5/2) d[IF5]/dt = ( -5/2) ( -0.47) = 1.175
torr /min**

**total Pressure rate change is addig all three d[IF5]/dt
+ d[I2] /dt + d[F3]/dt**

** = -0.47 + 0.235 + 1.175 = 0.94
torr /min**

The decomposition reaction given below: 2 IF5(g) 1 I2(g) + 5
F2(g) is carried out in a closed reaction vessel. If the partial
pressure of IF5(g) is decreasing at the rate of 144 torr/min, what
is the rate of change of the total pressure in the vessel? Delta
Ptot /delta t = ___torr/min

(a) Consider the combustion of ethylene, given below.
C2H4(g) + 3
O2(g) ? 2 CO2 (g) + 2
H2O (g)
If the concentration of C2H4 is decreasing
at the rate of 0.26 M/s, what are the rates of change in
the concentrations of CO2 and H2O?
CO2
(b) The rate of decrease in N2H4 partial
pressure in a closed reaction vessel from the following reaction is
41 torr/hr.
N2H4 (g) + H2
(g) ? 2 NH3 (g)
What are the...

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)...

14.7 g of butane (58.12 g/mol) undergoes combustion according to
the following equation. What pressure of carbon dioxide in atm is
produced at 318 K in a 1.58 L flask. 2 C4H10 (g) + 13 O2 (g) → 8
CO2 (g) + 10 H2O (g)

19.4 g of butane (58.12 g/mol) undergoes combustion according to
the following equation. What pressure of carbon dioxide in atm is
produced at 309 K in a 1.15 L flask.
2 C4H10(g) + 13 O2 (g) → 8
CO2 (g) + 10 H2O (g)

Butane, the fuel used in cigarette lighters, burns according to
the equation: 2 C4H10 (g) + 13 O2 (g) 8 CO2 (g) + 10 H2O(g) H =
– 5316 kJ a) Calculate the mass of oxygen that must react in order
for this reaction to generate 2150 kJ of heat b) Calculate the
amount of heat, including sign, that is transferred when 75.0 g of
butane react completely.

1. Given the values of So given below in J/mol K and
the values of ΔHfo given in kJ/mol, calculate
the value of ΔGo in kJ for the combustion of 1 mole of
butane to form carbon dioxide and gaseous water at 298 K.
S (C4H10(g)) = 273
S (O2(g)) = 208
S (CO2(g)) = 214
S (H2O(g)) = 189
ΔHfo (C4H10(g)) =
-123
ΔHfo (CO2(g)) = -394
ΔHfo (H2O(g)) = -223
2. A particular reaction has a ΔHo value...

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

Consider the reaction CO (g) + 0.5 O2 (g) -> CO2 (g). Compute
the molar delta H (in kJ/mol) for this reaction at 298 K and a
pressure of 30 bar. Joule-Thomson coefficients and heat capacities
are listed in the table below:
Compound
Cp (cal mol^-1 K^-1)
Joule-thomson coefficient
(K/bar)
CO
6.3423 + 0.0018363 T
1.20
O2
6.148 + 0.003102 T
1.15
CO2
6.369 + 0.0101 T
1.10

Consider the reaction CO (g) + 0.5 O2 (g) -> CO2 (g). Compute
the molar delta H (in kJ/mol) for this reaction at 298 K and a
pressure of 30 bar. Joule-Thomson coefficients and heat capacities
are listed in the table below:
Compound
Cp (cal mol^-1 K^-1)
Joule-thomson coefficient
(K/bar)
CO
6.3423 + 0.0018363 T
1.20
O2
6.148 + 0.003102 T
1.15
CO2
6.369 + 0.0101 T
1.10

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