I'm having trouble working out the energy changes....

[starbuckscoffee]

N2 + 3(H2)  <---------------->  2(NH3)

The reaction is propagated at a temperature of 500 °C and a pressure of 200 atm. Using the bond energies provided in the table, calculate the energy change for the conversion of one mole of nitrogen gas.

Enter your answers as integers.

a. Energy change in reaction:..................kJ

b. If 126.0 g of N2 gas is converted to NH3, the energy released is...........................kJ

For "a" i got 3364KJ but not sure if that's right

[Cthulhu]

What table?

[starbuckscoffee]

table

[Cthulhu]

CHM1031?

Anyway its a triple bond of and there is one mole.. 946kJ
and there are 3 Moles of and its a single bond(obviously) so 3mol *  436kJ/mol =1308kJ

946kJ+1308kJ = 2254kJ

I think

[starbuckscoffee]

cheers,yea haahaahha

[crayolé]

Is this unit 4 stuff?

[m@tty]

Is this unit 4 stuff?

I don't know if there is something similar in unit 4, but this is a uni question, if you didn't already realise.

[Potter]

Yeah, you do enthalpy in unit 4.