In a combination reaction, 1.62 g of lithium is mixed with 6.80 g of oxygen.

(b) How many moles of product are formed?

(c) After this reaction, how many grams of each reactant and product are present

Li - ?

O2 - ?

Li2O - ?

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

1. they vary with a higher number because boiling is way hotter than melting

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