a. From the equation of the reaction: 2 moles of CuSO4 need 4 moles of KCN. 3.7 moles will require: 4 / 2 * 3.7 = 7.4 moles of KCN
b. Moles of cyanogen = moles of CuSO4 * 1 / 2 = 1.75 / 2 = 0.875 moles
c. Moles of K2SO4 formed = moles of CuSO4 reacted = 5.25 moles
d. Moles of KCN = 2 * moles of CuSO4 = 2 * 2.5 = 5 moles
Mass = moles * molar mass = 5 * (39 + 12 + 14) = 325 g
e. Moles of cyanogen = 0.5 * moles of CuSO4 = 0.5 * 3.5 = 1.75 moles
Mass = moles * molar mass = 1.75 * (2 * 12 + 2 * 14) = 91 g
f. Moles of KCN = mass of KCN / molar mass = 45.3 / 65 = 0.697 moles
Moles of cyanogen = 1 / 4 * moles of KCN = 1/ 4 * 0.697 = 0.174 moles
Mass of cyanogen = moles * molar mass = 0.174 * 42 = 7.308 g
b. Determine what mass of rust can be removed by 540 g of oxalic acid? . Cyanogen, C2N2 is a colorless, poisonous gas that can be prepared by the following: +2 CuCN (a) CN2(+2 K,SO4 (ag) 2 CuSO4 () +4 KCN (a) o a. Determine how many moles of KCN are required to react with 3.7 moles of CuSO4 b. Determine how many moles of cyanogen are produced from 1.75 moles of CuSO4 c. Determine how many moles of K2SO4...
please help on all questions in the pics... numbers: b, c, d, e, f 3. A student collected the following data in the laboratory. mass of flask, g 52.87 mass of flask and sample, g 53.42 concentration of NaOH solution, M 0.101 initial buret reading, mL 23.78 final buret reading, mL Lab 9: Determining Ascorbic Acid in Vitamin C Tablets (b) what volume, in liters, of NaOH solution was used in the titration? O.101 X23.78 4.80356 Mb O.50 (c) How...