The reaction was studied at a series of different temperatures. A plot of ln(k) vs. 1/T gave a straight line relationship with a slope of -795 and a y-intercept of -0.561. Additionally, a study of the concentration of A with respect to time showed that only a plot of ln[A] vs. time gave a straight line relationship. What is the initial rate of this reaction when [A] = 0.673 at 280 K?

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

the answer is 1 i believe