Calculate AH°rxn from AH°7 values (use table in textbook appendix) a) Cl2 (g) + 2 Na (s) -› 2 NaCl (s) EITHER -411.1kJ/mol b) 2
H2S (g) + 3 02 (g) -> 2 SO2 (g) + 2 H20 (g)
1 answer:
To find AH°rxn, we use the following equation:
What we're going to do is to sum the enthalpy of the products and then substract with the enthalpy of the reactives:
As you can see, we need to multiply by the coefficients of the reaction.
Now, just replace the values of the table:
So the answer is -822.2kJ/mol.
For b:
Now, just replace the values of the table:
The answer for b is -1036kJ/mol.
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Answer:
The enthalpy change of the reaction is -66.88 kJ/mol.
Explanation:
Mass of the solution = m = 100 g
Heat capacity of the solution = c = 4.18 J/g°C
Initial temperature of the solutions before mixing =
Final temperature of the solution after mixing =
Heat gained by the solution due to heat released by reaction between HCl and silver nitrate = Q
Heat released due to reaction = Q' =-Q = -334.4 J
Moles of silver nitrate = n
Molarity of silver nitrate solution = 0.100 M
Volume of the silver nitrate solution = 50.0 mL = 0.050 L ( 1 mL = 0.001 L)
Enthalpy change of the reaction =
1 J = 0.001 kJ
The enthalpy change of the reaction is -66.88 kJ/mol.