The second-order rate constant for the following gas-phase reaction is 0.0442 mol L^-1 s^-1. We start with 0.135 mol C2F4 in a 2.00 liter container, with no C4F8 initially present.
2 C2F4(g) → C4F8 (g)
What will be the concentration of C2F4 after 1 hour?
What will be the concentration of C4F8 after 1 hour?
What is the half-life of the reaction for the initial C2F4 concentration given above?
How long will it take for half of the C2F4 that remains after 1 hour to disappear?

Answer the questions about this reaction: nai(aq) + cl2(g) → nacl(aq) + i2(g) write the oxidation and reduction half-reactions: oxidation half-reaction: reduction half-reaction: based on the table of relative strengths of oxidizing and reducing agents (b-18), would these reactants form these products? write the balanced equation: answer options: a. 0/na -> +1/na+1e- b. nai(aq) + cl2(g) → nacl(aq) + i2(g) c. +1/na+1e- -> 0 /na d. -1/2i -> 0/i2+2e- e. no f. 4nai(aq) + cl2(g) → 4nacl(aq) + i2(g) g. 2nai(aq) + cl2(g) → 2nacl(aq) + i2(g) h. 4nai(aq) + 2cl2(g) → 4nacl(aq) + 2i2(g) i. nai(aq) + cl2(g) → nacl(aq) + i2(g) j. 0/cl2+2e -> -1/2cl- k. yes