Question

Thermochemistry

Answer 1

When 8.50g of \[NH _{3}\] are formed, according to the following \[N _{2}(g) + 3H _{2}(g) --> 2NH _{3} \] 23.1kJ of heat are released.
A) How many kJ of heat are released when 1 mol of N2 reacts with xcess H2?

Answer 2

B) How many kJ of heat are released when 2 mol of NH3 are formed?
C) How many kJ of heat are released when 4 mol of N2 reacts with 4 mol of H2

Answer 3

On A) I thought because the equation says 1 N2 then the answer to that one would be 23.1?? ....
then on B) converting 8.5 g of NH3 to moles is .5 sooo to get 2 mols you would multiply by 4? so multiply 23.1 by 4?
C) and 4 mols of N2 on this one sooo 4 x 23.1?

Answer 4

1st is wrong

Answer 5

how?

Answer 6

but for one mole of N2 is ok but energy relaesed is for the 8.5 gram of NH3 formed if you back convert how much of N2 is required to produce the 8.5 gram of NH3 u will find it

Answer 7

first convert weight of NH3 8.5 gram to moles

Answer 8

I did that already

Answer 9

sory getting confused let me know

Answer 10

then fine

Answer 11

i just can't think where to go from there?
I know my answers are wrong ... except b might be right ... but I'm too tired to get this stuff