Use the data given to calculate the value of delta G rxn for the reaction at 25C
2C(graphite)+H2(g)--->C2H2(g)
C H2 C2H2
S(J K^-1 mol^-1)| 5.74 |130.68| 201.0
-------------------
delta H(kJ/mol) | 0 | 0 |-226.8
a.-291.4 kj
b.-244.3 Kj
c.-226.8 kj
d.-207.6 Kj
e.-64.6 Kj
Tables, spaces, and the like don't do well on the board. You need to find another format that doesn't require spaces or tables.
Use the data given to calculate the value of delta G rxn for the reaction at 25C
2C(graphite)+H2(g)--->C2H2(g)
C______H2_______C2H2___________________5.74| 130.68| 201.0 | S (JK^-1mol^-1)
_______________________________________
0 | 0 | -226.8|delta H(KJ/mol)
a.-291.4 kj
b.-244.3 Kj
c.-226.8 kj
d.-207.6 Kj
e.-64.6 Kj
Thanks for trying but I don't see an improvement over the previous version.
I cant figure out how to do a table :(
Use the data given to calculate the value of delta G rxn for the reaction at 25C
2C(graphite)+H2(g)--->C2H2(g)
C= S(J K^-1) => 5.74 and delta H(kJ/mol)=>0
H2= S(J K^-1)=> 130.68 and delta H (kJ/mol)=>0
C2H2= S(J K^-1)=> 201.0 and delta H(kJ/mol)=> -226.8
a.-291.4 kj
b.-244.3 Kj
c.-226.8 kj
d.-207.6 Kj
e.-64.6 Kj
To calculate the value of ΔG_rxn (the change in Gibbs free energy) for the given reaction, we can use the equation:
ΔG_rxn = ΔH_rxn - TΔS_rxn
where ΔH_rxn is the change in enthalpy and ΔS_rxn is the change in entropy, and T is the temperature in Kelvin.
Given data:
ΔH(C) = 0 kJ/mol
ΔH(H2) = 0 kJ/mol
ΔH(C2H2) = -226.8 kJ/mol
S(C) = 5.74 J/(K mol)
S(H2) = 130.68 J/(K mol)
S(C2H2) = 201.0 J/(K mol)
T = 25°C = 298 K
To calculate ΔH_rxn, we need to find the difference in the enthalpy between the products and the reactants. Since we have only one reactant (C(graphite) and H2(g)) and one product (C2H2(g)), we can calculate ΔH_rxn as follows:
ΔH_rxn = ΣΔH(products) - ΣΔH(reactants)
= ΔH(C2H2) - [ΔH(C) + ΔH(H2)]
= -226.8 kJ/mol - [0 kJ/mol + 0 kJ/mol]
= -226.8 kJ/mol
To calculate ΔS_rxn, we need to find the difference in entropy between the products and the reactants, following the same approach:
ΔS_rxn = ΣΔS(products) - ΣΔS(reactants)
= ΔS(C2H2) - [ΔS(C) + ΔS(H2)]
= 201.0 J/(K mol) - [5.74 J/(K mol) + 130.68 J/(K mol)]
= 201.0 J/(K mol) - 136.42 J/(K mol)
= 64.58 J/(K mol)
Now, substituting the values into the equation:
ΔG_rxn = ΔH_rxn - TΔS_rxn
= -226.8 kJ/mol - (298 K)(64.58 J/(K mol))
To perform the unit conversion, we need to convert kJ to J and then calculate ΔG_rxn:
ΔG_rxn = -226.8 kJ/mol - (298 K)(64.58 J/(K mol))
= -226.8 * 1000 J/mol - 19011.8 J/mol
= -226800 J/mol - 19011.8 J/mol
= -245811.8 J/mol
Finally, we convert J/mol to kJ/mol:
ΔG_rxn = -245811.8 J/mol / 1000
= -245.8118 kJ/mol
Therefore, the value of ΔG_rxn for the reaction at 25°C is approximately -245.8 kJ/mol.
The correct option would be:
b. -244.3 kJ