The Green Chemistry movement strives to replace hazardous oxidizers, such as chlorine, with innocuous oxidizers such as hydrogen peroxide. Exercise 2.26 describes the Bayer process for synthesizing hydrazine, N_2H_4. For hydrazine synthesis by green chemistry, the overall reaction is as follows. 2NH_3 + H_2O_2 rightarrow N_2H_4 + 2H_2O In this modified process, only two synthesis steps are required. The first step is conversion of acetone, CH_3C(O)CH_3, to acetazine, (CH_3)_2C=N-N=C(CH_3)_2, in aqueous solution at 50 degree C. H_2O_2 + 2CH_3C(O)CH_3 + 2NH_3 rightarrow (CH_3)_2C=N-N=C(CH_3)_2 + 4H_2O The second step is the hydrolysis of acetazine into hydrazine and acetone in aqueous solution at 50 degree C. hydrolysis: (CH_3)_2C=N-N=C(CH_3)_2 + 2H_O rightarrow N_2H_4 + 2CH_3C(O)CH_3 The hydrazine is distilled from the aqueous solution as a hydrate, N_2H_4 middot H_2O. Design a process to produce hydrazine hydrate from ammonia and hydrogen peroxide. The hydrogen peroxide is available as a mixture of 70% hydrogen peroxide in 30% water. a. Use the chemical formulas C_3H_6O for acetone and C_6 H_12 N_2 for acetazine. b. You may assume if acetone and ammonia are in excess in the acetazine synthesis, the H_2O_2 is completely consumed. c. You may assume if H_2O is in excess in the acetazine hydrolysis, the acetazine is completely consumed. d. You may assume all substances in this exercise are soluble in water.