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

Mass is conserved in a chemical reaction, which of these is TRUE about the mass of the products?  *1 pointless than the mass of the reactantsequals to the mass of the reactantgreater than the mass of the reactantsnot related to the mass of the reactants

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%.

The chemical reaction below: (SELECT ALL APPLICABLE STATEMENTS)H(NO3) + Cu --> Cu(NO3)2 + NO2 + H2OResponsesIs not in violation of the Law of Conservation of MatterIs not in violation of the Law of Conservation of MatterRepresents a balanced chemical equationRepresents a balanced chemical equationRepresents an unbalanced chemical equationRepresents an unbalanced chemical equationRepresents a decomposition reactionRepresents a decomposition reactionIs in violation of the Law of Conservation of MatterIs in violation of the Law of Conservation of MatterRepresents a synthesis reaction

The law of conservation of mass states that: Mass can be destroyed in a chemical reactionMass can be created in a chemical reactionMass is conserved in a chemical reactionSave