Respuesta :
Answer: The value of [tex]\Delta H[/tex] for the reaction will be -854.4 kJ
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Given mass of barium = 5.00 g
Molar mass of barium = 137.33 g/mol
Putting values in above equation, we get:
[tex]\text{Moles of barium}=\frac{5.00g}{137.33g/mol}=0.0364mol[/tex]
For the given chemical reaction:
[tex]Ba(s)+Cl_2(g)\rightarrow BaCl_2(s)[/tex]
By Stoichiometry of the reaction:
1 mole of barium produces 1 mole of barium chloride
So, 0.0364 moles of barium will produce = [tex]\frac{1}[1}\times 0.0364=0.0364mol[/tex] of barium chloride
We are given:
Energy released for 0.0364 moles of barium chloride formed is 31.1 kJ
Now, calculating the heat when 1 mole of barium chloride is produced.
By Stoichiometry of the reaction:
When 0.0364 moles of barium chloride is produced, the energy evolved is 31.1 kJ
So, when 1 mole of barium chloride is produced, the energy evolved will be = [tex]\frac{31.1kJ}{0.0364mol}\times 1mol=854.4J[/tex]
Sign convention of heat:
When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.
Hence, the value of [tex]\Delta H[/tex] for the reaction will be -854.4 kJ
