Completely ****ed up the born haber cycle, honestly no idea how or why I got +1910 or something Stupid mistakes
I got the same as you originally but when I went back, I forgot to multiply the ionisation Enthalpy by 2 and that's how I got 2000 something so I'm sure you didn't multiply it by 2
It wanted standard enthalpy change, hence you do it for one mole hence you divide answers by 2 I believe (that's what happened on a previous mark scheme)
I'm pretty sure it just asked for the enthalpy change for the reaction, and they provided you with the standard enthalpy changes for 1 mole, so I think you had to multiply the values by 2 not divide by 2.
Hi I have some questions and answers if anyone wants to add to it?
Lattice dissociation of K2O being less endothermic than Na2O:
K+ ions are bigger than Na+ ions Weaker electrostatic force of attraction between K+ and O2- ions/weaker ionic bonding Less energy needed to break the ionic lattice
Solubility of MgCl2 decreases Forward reaction is exothermic Equilibrium shifts left to oppose increase in temperature
Enthalpy of solution = -155 kJ/mol
Question stated that solubility is defined as the amount of solid able to dissolve in water, so as it is an endothermic reaction, more MgCl2 is produced if you increase temperature, hence solubility is increased
Hi I have some questions and answers if anyone wants to add to it?
Lattice dissociation of K2O being less endothermic than Na2O:
K+ ions are bigger than Na+ ions Weaker electrostatic force of attraction between K+ and O2- ions/weaker ionic bonding Less energy needed to break the ionic lattice
Solubility of MgCl2 decreases Forward reaction is exothermic Equilibrium shifts left to oppose increase in temperature
Enthalpy of solution = -155 kJ/mol
for the lattice dissociation question i put na+ ions were smaller and that there is a stronger attraction between the molecules, would i still get the marks???