Which of the following statement is incorrect about the equation? C_(2)H_(5)OH(l)+3O_(2)(g) to 2CO_(2)(g)+3H_(2)O(l),Delta_(r)H^(-)=-1367" kJ "mol^(-1)

Which of the following statement is incorrect about the equation? C_(

1.	Which of the following statement is incorrect about the equation? C_(2)H_(5)OH(l)+3O_(2)(g) to 2CO_(2)(g)+3H_(2)O(l),Delta_(r)H^(-)=-1367" kJ "mol^(-1)
Answer» the reaction is endothermic in nature. The numerical value of `Delta_(r)H^(ө)` refers to the number of moles of SUBSTANCES specified by an equation. Standard enthalpy change `Delta_(r)H^(ө)` will have units as kJ `mol^(-1)` The coefficients in a balanced thermochemical equations refer to the number of moles (never molecules) of reactants and products involved in the reaction The equation describes the combustion of liquid ETHANOL at constant temperature and pressure. Solution :`C_(2)H_(5)OH(l)+3O_(2)(g)to2CO_(2)(g)+3H_(2)O(l)` `Delta_(r)H=-1367" kJ "mol^(-1)` The above equation describes the combustion of liquid ethanol at constant temperature and pressure. The negative sign of enthalpy change INDICATES that this is an exothermic reaction.