Answer:
The reaction proceeds with a net release of free energy.
Explanation:
Exergonic reactions: It is known as the chemical reaction where the change in the free energy is occur negative or there is a net release of free energy, and indicating a spontaneous reaction. For the processes this takes place under constant temperature, and pressure conditions.
The Gibbs free energy is used whereas the processes which takes place under constant volume, and temperature conditions, and their Helmholtz energy is used. Cellular respiration is the example of an exergonic reaction.
Answer:
V= 8.235 ml
Explanation:
The man above me copied me from the comments
I did it >:C
The value of ΔG° (gibbs free energy change) is -2703kj and -2657kj.
Given ,
combustion reaction of butane :
C4H10(g) + 13/2O2 (g) →4CO2(g) + 5H2O(g)
Method-1 :
We know ,
ΔGrxn = sum of ΔG (product ) - sum of ΔG (reactant )
= [4 × (-394.4) + 5×(-228.6) ] - [1×(-16.7)]
ΔGrxn = -2720.6kj
Method-2 :
We know ,
ΔG = ΔH -TΔS
T =298K
Thus , ΔHrxn = sum of ΔH (product ) - sum of ΔH (reactant )
= [4×(-393.5) + 5×(-241.8) ] - [ 1×(-126)]
ΔHrxn = -2657kj
ΔSrxn = sum of ΔS (product ) - sum of ΔS( reactant )
= [ 4×(213.7) + 5×188.7 ] - [ 13/2 ×205 + 1×310 ]
ΔSrxn = 155.8j/K
ΔSrxn = 0.1558kj/K
Thus , ΔG = ΔH - TΔS
= -2657 - ( 298 × 0.1558kj/K )
ΔG = -2720kj
Hence , the value of ΔG is -2703kj .
Learn more combustion reaction here :
brainly.com/question/13251946
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The heat of combustion for methanol is 727 kj/mol
<em><u>calculation</u></em>
calculate the moles of methanol (CH3OH)
moles = mass/molar mass
molar mass of methanol = 12 +( 1 x3) +16 + 1= 32 g /mol
moles is therefore= 64.0 g / 32 g/mol = 2 moles
Heat of combustion is therefore = 1454 Kj / 2 moles = 727 Kj/mol
