A 31.2 gram sample of C6H6 (benzene) is reacted with excess HNO3 (nitric acid). 36.0 grams of the desired product, nitrobenzene C6H5NO2, is isolated from this reaction. Water is the by-product.
A. Write a balanced chemical equation for this reaction
B. What is the percent yield of nitrobenzene?
A 31.2 gram sample of C6H6 (benzene) is reacted with excess HNO3 (nitric acid). 36.0 grams...
benzoin: .40g and 1.5 ml of nitric acid, to prepare benzil. you isolated .260g of pure benzil product after recrystallization. (Density of HN03= 1.42 g/mL) 1. write a balanced chemical equation for the reaction 2. create a stoichiometry table and calculate the limiting reagent in this reaction 3. calculate the theoretical yield and percent yield of the product
How many grams of nitric acid, HNO3, are required to neutralize (i.e. completely react with) 3.33 moles of Ca(OH)2 according to the balanced chemical reaction: 2HNO3 + Ca(OH)2 --> 2H2O + Ca(NO3)2
In lab, you reacted copper metal with aqueous nitric acid to produce aqueous Copper (11) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) + 2NO2 (g) + 2H20 (1) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...
In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...
In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...
When nitrogen dioxide from car exhaust combines with water in the air, it forms nitric acid (HNO3) which causes acid rain and nitrogen monoxide. a.Write a balanced chemical equation for the reaction above. b.How many moles of each product are produced from 0.250 moles of water? c.How many grams of nitrogen dioxide are needed to form 75.0 g of nitric acid?
Concentrated nitric acid (HNO3) can oxidise elemental sulfur (S) to give sulfur dioxide, nitrogen dioxide and water, write a balanced chemical equation for this process.
Write an equation for the reaction that takes place between nitric acid, HNO3, and ammonia, NH3, when aqueous solutions of the two are mixed. Write the product in ionized form, but the reactants in molecular form. It is not necessary to include states such as (aq) or (g). _____+______-->_____+______ Write a balanced molecular equation for the reaction that occurs when aqueous solutions of hydrobromic acid, HBr, and potassium hydroxide, KOH, are combined. It is not necessary to include states such...
) sulfide reacts with nitric acid according to the reaction below: 5. Antimony(III) sulfide reacts w Sb2S3(s) + 10 HNO3(aq) → Sb2Os(5) a. Calculate the theoretical yield in sulfide reacts with 0.579 mol nitric acid. O HNO3(aq) Sb Os(s) + 10 NO(g) + 3 S(s) + 5 H200 clical yield (in grams) of each product when 32.1 g of antimony(1) 321 gs bz63 x 1 mol sbg 82 x mol sbag Molsb2S₃ 0.519 HNO3 x 01 Slezs - Imolsberg Omo...
Exp 210 CYCLE OF COPPER REACTIONS Part 1: Reaction of solid copper with concentrated nitric acid Observations: (partial example given) Tke copper wire was bright/shiny after cleaning wits steel wool. The nitric acia solution. was nearly clear/coloriess olthongh α very faint reddish brown discoloration was evident. Reaction Products The cemplet d Balanced molecular chemical equation (this first reaction equation is given as an example) What ions are in solution after the reaction is complete? What is the oxidation state of...