Assuming that the specific heat of the solution is 4.18 j/(g⋅∘c), that its density is 1.00 g/ml, and that the calorimeter itself absorbs a negligible amount of heat, calculate δh in kilojoules for the reaction. h2so4(aq)+2naoh→2h2o(l)+na2so4(aq)

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