Water forms according to the equation below: 2h2(g) + o2(g) jpg 2h2o(g) hrxn = -483.64 kj how much energy is released during the formation of 1 mol h2o(g)? kj

Answer : The amount of energy released is, -241.82 KJ

Explanation : Given,

The balanced chemical reaction is,

From this we conclude that,

As, 2 moles of released amount of energy = -483.64 KJ

So, 1 mole of released amount of energy =

Therefore, the amount of energy released is, -241.82 KJ

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g