When `MgO` reacts with `H_(2)O` at `25^(@)C` and 1 atm, the volume change is `-4.6mL. mol^(-1).`
`MgO(s)+H_(2)O(l)toMg(OH)_(2)(s)`
What is the value of `deltaH- deltaE` for this reaction?

Mg(s)+H_(2)O(l) overset("warm")toMg(OH)_(2)+H_(2)uarr

Mg(s)+H_(2)O(l) overset("warm")toMg(OH)_(2)+H_(2)uarr

Mg(s)+H_(2)O(l) overset("warm")toMg(OH)_(2)+H_(2)uarr

Which of the given statements is (are) correct about the following reaction ? MgO(s) + H_(2)O(l) to Mg(OH)_(2)(s) + heat

The heat of reaction for the following reaction (DeltaH^(0)) at 25^(@)C temperatue is -1368 kJ: C_(2)H_(5)OH(l)+3O_(2)(g) to 2CO_(2)(g)+3H_(2)O(l) If the enthalpy of formation of CO_(2)(g) and H_(2)O(l) at 25^(@)C are -393.5 and -285.8 kJ*mol^(-1) respectively, then what will be the value of the standard enthalpy of formation of C_(2)H_(5)OH(l) ?

H_(2)O(s) rarr H_(2)O(l), DeltaH = 6.01 kJ DeltaH is the heat of …………………of ice.

H_(2)O(s) rarr H_(2)O(l), DeltaH = 6.01 kJ DeltaH is the heat of …………………of ice.

H_(2)O(l) rarr H_(2)O(s), DeltaH =- 6.01 kJ DeltaH is the heat of ……………….of water.