posted by jamie on .
Determine the amount of heat (in kJ) given off when 2.07 multiplied by 104 g of ammonia are produced according to the following equation. Assume that the reaction takes place under standard-state conditions at 25.0°C.
N2(g) + 3 H2(g) 2 NH3(g) ΔH°rxn = -92.6 kJ
You didn't write an arrow. Without an arrow we can't tell the difference between the products and the reactants. I will place the arrow where I think it goes but you correct me if I'm wrong.
N2(g) + 3H2(g) ==>2NH3(g)
So 92.6 kJ of heat are produced to form how many grams of NH3? Would that be 2 x molar mass = 2 x 17 = 34 g NH3?
Then 92.6 kJ x (2.07 x 10^4/34) = ??
Check my thinking. Check my typing.
Yes you had the equation right. And that worked.