If melting one mole of ice to water requires $6$ kJ of enthalpy, then freezing of water to two mole of ice will require ________ kJ of energy.

Question

If melting one mole of ice to water requires 6  kJ of enthalpy- then freezing of water to two mole of ice will require - kJ of energy-126-12-6

Toppr Admin · Accepted Answer

Melting one mole of ice to water-x2192-6kjMelting 2 moles of ice to water-x2192-12kjIf the reaction is reversed i-e- freezing of water to two moles of ice- energy required would be multiplied with -x2212-1- - here it would be -x2212-12kjIt is beacuse enthalpy is a state function-

If melting one mole of ice to water requires $6$ kJ of enthalpy, then freezing of water to two mole of ice will require ________ kJ of energy.
$12$
$6$
$- 12$
$- 6$

Melting one mole of ice to water $\to 6 k j$
Melting 2 moles of ice to water $\to 12 k j$
If the reaction is reversed i.e. freezing of water to two moles of ice, energy required would be multiplied with $(- 1)$ , here it would be $- 12 k j$
It is beacuse enthalpy is a state function.

If melting one mole of ice to water requires 6 kJ of enthalpy, then freezing of water to two mole of ice will require ________ kJ of energy.126−12−6

Melting one mole of ice to water→6kjMelting 2 moles of ice to water→12kjIf the reaction is reversed i.e. freezing of water to two moles of ice, energy required would be multiplied with (−1) , here it would be −12kjIt is beacuse enthalpy is a state function.

If melting one mole of ice to water requires $6$ kJ of enthalpy, then freezing of water to two mole of ice will require ________ kJ of energy.
$12$
$6$
$- 12$
$- 6$

Melting one mole of ice to water $\to 6 k j$
Melting 2 moles of ice to water $\to 12 k j$
If the reaction is reversed i.e. freezing of water to two moles of ice, energy required would be multiplied with $(- 1)$ , here it would be $- 12 k j$
It is beacuse enthalpy is a state function.