The hydrogenation of ethene gas under standard conditions (T = 298K) shows a decrease in disorder (ΔS* = -120.7 J/(mol m*K)) during an exothermic reaction (ΔH* = -136.9 kJ/mol).
C_2H_4 (g) + H_2 (g) > C_2H_6 (g)
a. Explain how you would have predicted the sign of ΔS* for this reaction.
b. Explain what is happening to the disorder of the surroundings.
c. Determine whether the reaction is spontaneous or nonspontaneous by calculating ΔG°.
d. How would the spontaneity of the reaction change with an increase in temperature? Explain.

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 75.0%.