Question

ΔH for the formation of CuCl2 from its elements is -220.1 kJ/mol. How many kJ are associated with the formation of 0.30 mole of CuCl2?

-66 kJ
-78 kJ
85 kJ
201 kJ

Answer 1

0.3 * - 220.1 = - 66.03kJ

Answer 2

`\Delta _fH=-66.03kJ`

Step-by-step explanation:

Hello,

In this case, by knowing the enthalpy of formation of the copper (II) chloride is -220.1kJ/mol and there are 0.3 moles of such compound, the resulting whole energy is obtained by multiplying those values as the moles define the total energy as shown below:

`\Delta _fH=-220.1(kJ)/(mol)*0.30mol\\ \Delta _fH=-66.03kJ`

Best regards.