Question

1. The compound thiophene contains carbon, hydrogen and sulfur. When a sample weighing 2.450 g is subjected to complete combustion analysis with oxygen, 5.126 g of carbon dioxide and 1.049 g of water are produced. What is the simplest formula of thiophene? 2. When zinc metal reacts with copper(II) nitrate, zinc(II) nitrate and copper metal are the products. How many grams of zinc metal are required to react completely with 725 mL of 0.1955 M copper (II) nitrate solution? What mass of copper metal is produced? You will need a balanced equation to solve this problem! 3. One step in the process of manufacturing nitric acid (HNO3), a staple industrial chemical, is 3 NO2 (g) + H20 (1) ► 2HNO3(aq) + NO(g) Starting with 1.55 kg NO2 and 0.355 kg of water, calculate the theoretical yield of nitric acid in grams. When the experiment is run, the actual yield of nitric acid is found to be 0.894 kg. What is the limiting reactant? What is the percent yield of the reaction?

for the first question, simple formula is referring to empircial formula

Answer 1

Ansser Molar mass C8/mas) 44.01 12.01 H20 1.008 H 32.06 mass molar mars of moles Number 1 mol f C 1. mol of Co Cantains S.126 moles of c 5.126 of Co2 S.126 moles af Co2 14.01 4.01 0.1165 moles of C .. Mass of c in Cmpouna(o.1165x 12-61)3 = 1-399 8 mol of H2o Cntains 2 moles of H 1 1.049 of H2o= 1.049 1.049 moles of H2O moles of H - 2X 18-62 18-02 0.1164 maleA of H mass of H in Cmpound - (o.1164X 1.008) 3-0.11738 of s in Cmpouna- 2-4 50- (1.399 + 0.1173) a MAss =0.9337 Moles of S in Cmpound 0.9337 moles - 0.02912 moles 32-06

Ratio of moles of C H: S- 0.1165 0.1l64 : 0.02912 0.1169 O.1165 1 13 O.02912 0.02912 4:4:1 So Simplest formula of thiophene is Ca H4s 2