Now consider a similar process. use the same initial conditions for the copper, but assume that the h2o is initially in the gas phase at 100 °c. i. sketch two temperature vs. energy-added diagrams, one for each substance, and mark the initial state for each one. ii. how can you determine if the h2o will undergo a temperature change? (what calculations and comparisons – think energy – would you need to make? don’t actually do the calculations; just explain what you would need to do.)

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