Calculate the enthalpy of formation (kJ/mol) of MgO(s). The enthalpy of reaction for the equation as written is 100.8 kJ/mol. If the answer is negative, enter the sign and then the magnitude.

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Calculate the enthalpy of formation (kJ/mol) of MgO(s).The enthalpy of reaction for the equation as written is -100.8 kJ/mol. If the answer is negative, enter the sign and then the magnitude.

Given:  

,

The enthalpy of formation of MgO(s) is -601.7 kJ/mol

Explanation:

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles.

The equation used to calculate enthalpy change is of a reaction is:

For the given chemical reaction:

The equation for the enthalpy change of the above reaction is:

We are given:

Putting values in above equation, we get:

Hence, the enthalpy of formation of MgO(s) is -601.7 kJ/mol

im pretty sure its b

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.