Thermochemistry question part (2)
Posted: Tue Jun 29, 2021 11:03 pm
1]Consider the following balanced reaction:
\(2A_2 + 3B \rightarrow C_2 + 2D \)
What is the enthalpy of reaction if the enthalpy of formation of the compounds is given as
\(A_2 = 7.78 kJ/mol; B = -18.43 kJ/mol; C_2 = 0 kJ/mol; D = 9.96 kJ/mol.\)
Record your answer in scientific notation using 3 significant figures.
My answer to this question is 59.65 kJ/mol computed as follows: [9.96*2-2*(7.78)-3*(-18.43)=59.65]
2]Calculate ΔH° for the process Co3O4(s) → 3 Co(s) + 2 O2(g)
from the following information
Co(s) + ½ O2(g) → CoO(s) ΔH° = -120.6 kJ/mol
3 CoO(s) + ½ O2(g) → Co3O4(s) ΔH° = -632.4 kJ/mol
I am working on these two questions. Any chemistry help will be accepted.
\(2A_2 + 3B \rightarrow C_2 + 2D \)
What is the enthalpy of reaction if the enthalpy of formation of the compounds is given as
\(A_2 = 7.78 kJ/mol; B = -18.43 kJ/mol; C_2 = 0 kJ/mol; D = 9.96 kJ/mol.\)
Record your answer in scientific notation using 3 significant figures.
My answer to this question is 59.65 kJ/mol computed as follows: [9.96*2-2*(7.78)-3*(-18.43)=59.65]
2]Calculate ΔH° for the process Co3O4(s) → 3 Co(s) + 2 O2(g)
from the following information
Co(s) + ½ O2(g) → CoO(s) ΔH° = -120.6 kJ/mol
3 CoO(s) + ½ O2(g) → Co3O4(s) ΔH° = -632.4 kJ/mol
I am working on these two questions. Any chemistry help will be accepted.