How much energy would be produced from the reaction of 2.40 moles hydrogen with 3.95 moles chlorine? ___ H2 + ___ Cl2 ___ HCl ΔH = -554 kJ

How much energy would be produced from the reaction of 2.40 moles hydrogen with 3.95 moles chlorine?

Explanation:

Given,

2.40 moles hydrogen reacts with 3.95 moles chlorine.

From the balanced chemical equation,

1mol. of H2 reacts with 1mol. of Cl2

then,

2.40mol. of H2 reacts with ----?mol of Cl2

So, the remaining moles of Cl2 is in excess.

The limiting reagent is--- H2.

1mol. of H2 releases --- 554kJ of energy

then,

2.40mol of H2 releases ---- ?

Answer is: deltaH =-1329.6kJ

c is the answer because when something is left after something evaporates that shows the chemical change.

(b) which contains higher levels of vitamin b, oranges or spinach?

explanation:

you can eliminate a, c, and d because they are questions based on opinions.