Consider the reaction shown in the following balanced equation:2 Cu2S (s) + 3 O2 (g) → 2 Cu2O (s) + 2 SO2 (g)You have 1.00 mole each of Cu2S and O2.How many moles of Cu2O can be produced if 1.00 mole of Cu2S reacts? Answer 1 Question 1How many moles of Cu2O can be produced if 1.00 mole of O2 reacts? Answer 2 Question 1The amount of Cu2O that can be produced is smaller from 1.00 mole of Answer 3 Question 1 than the other reagent. Therefore, Answer 4 Question 1 is the limiting reagent and Answer 5 Question 1 is the reagent in excess when 1.00 mole of each is available.  Consider instead that you have 1.00 g each of Cu2S (molar mass of Cu2S is 159 g mol−1) and O2 (molar mass of O2 is 32.0 g mol−1).1.00 g of Cu2S is Answer 6 Question 1 moles of Cu2S and would produce Answer 7 Question 1 moles of Cu2O if all the Cu2S reacts. 1.00 g of O2 is Answer 8 Question 1 moles of O2 and would produce Answer 9 Question 1 moles of Cu2O if all the O2 reacts.The amount of Cu2O that can be produced is smaller from 1.00 g of Answer 10 Question 1 than the other reagent. Therefore, Answer 11 Question 1 is the limiting reagent and Answer 12 Question 1 is the reagent in excess when 1.00 g of each is available.

Consider the reaction shown in the following balanced equation:2 Cu2S (s) + 3 O2 (g) → 2 Cu2O (s) + 2 SO2 (g)An excess of Cu2S is added to 8.25 x 10−2 moles of O2.If all of the O2 reacts, the amount of SO2 that can theoretically be produced is Answer 1 Question 2 moles or Answer 2 Question 2 g. Molar mass of SO2 is 64.1 g mol−1.The reaction was performed in a lab and only 3.27 g of SO2 was produced. The percentage yield for the experiment was Answer 3 Question 2%.

Use the balanced equation to answer the following questions.CuSO4(aq) + 2NaOH(aq) —->Cu(OH)2(s) + Na2SO4(aq)i. What is the ratio of moles of CuSO4 to moles of NaOH?ii. If 638.44 g CuSO4 reacts with 240.0 NaOH, which is the limiting reagent?iii. Using the limiting reagent to determine how many grams of Cu(OH)2 should precipitate out in the reaction.iv. If only 174.6g of Cu(OH)2 precipitate were actually collected from the reaction, what would the percent yield be?

The law of conservation of mass states that:The mass of products is greater than the mass of reactantsThe mass of products is less than the mass of reactantsThe mass of products is equal to the mass of reactantsThe mass of products can be either greater than or less than the mass of reactants2How many grams of copper oxide are produced during the following reaction (assuming it is complete)?: 2Cu (6.35 g) + O2 (1.60 g) → 2CuO7.95 g4.75 g6.35 g15.9 g3In a chemical reaction, the mass of products is often lower than expected. There are several explanations for why this might be the case. Which of the following is not a possible explanation?Some of the reactants may have reacted in different unexpected waysThe mass of the reactants is greater than the mass of the productsThe reaction may not have finishedSome of the product may have been lost during removal4Which of the following is a balanced equation for the formation of water from hydrogen and oxygen?2H2 + O2 → H2O2H2 + 2O2 → 2H2O2H2 + O2 → 2H2OH2 + O2 → H2O25Which of the following is a balanced equation for the reaction of hydrogen and chlorine?H2 + Cl2 → HCl2H + 2Cl → 2HClH2 + Cl2 → 2HClH + Cl → HCl

Copper carbonate, CuCO3, undergoes thermal decomposition to produce copper oxide, CuO, and carbon dioxide, CO2.When 24.7 g of CuCO3 was heated to constant mass, 15.9 g of CuO was produced.Determine the balanced equation for the reaction.CuCO3 → CuO + CO2CuCO3 → 2CuO + 2CO2CuCO3 → CuO + 2CO23CuCO3 → CuO + CO2I DON'T KNOWSUBMIT ANSWER

Classify the chemical equations as being balanced or not balanced.2CO + 2NO → 2CO2 + N26CO2 + 6H2O → C6H12O6 + O2H2CO3 → H2O + CO22Cu + O2 → CuO