Respuesta :
Answer: The value of [tex]\Delta H[/tex] for the reaction will be -55.48 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 copper (I) oxide = 54.08 g
Molar mass of copper (I) oxide = 143.1 g/mol
Putting values in above equation, we get:
[tex]\text{Moles of }Cu_2O=\frac{54.08g}{143.1g/mol}=0.380mol[/tex]
For the given chemical reaction:
[tex]2Cu_2O(s)+O_2(g)\rightarrow 4CuO(s);\Delta H^o_{rxn}=-292.0kJ[/tex]
By Stoichiometry of the reaction:
When 2 moles of copper (I) oxide reacts, the energy evolved is 292.0 kJ
So, when 0.380 moles of copper (I) oxide will react, the energy evolved will be [tex]\frac{292kJ}{2mol}\times 0.380mol=55.48kJ[/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 -55.48 kJ
