Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Write the two possible conversion factors that can be obtained from the molar mass for oxygen.
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- When 273.55 grams of water are produced, 1.5429 × 1025 particles of potassium hydroxide were reacted. What is the percent yield of this reaction?arrow_forwardAcid rain is caused in part by burning coal that contains sulfur impurities. The sulfur is converted first to SO2, which reacts with oxygen and atmospheric moisture to produce sulfuric acid, H2SO4. If a particular coal contains 1.90% sulfur (by mass), calculate the mass of sulfuric acid produced by burning a metric ton (1000 kg) of the coal.arrow_forwardReferences Use the References to access important values if needed for this question. For the following reaction, 24.3 grams of iron are allowed to react with 27.8 grams of hydrochloric acid. iron(s) + hydrochloric acid (aq) → iron (II) chloride (aq) + hydrogen (g) What is the maximum amount of iron(II) chloride that can be formed? Mass= g What is the FORMULA for the limiting reactant? What amount of the excess reactant remains after the reaction is complete? Mass= g Submit Answerarrow_forward
- Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/molarrow_forwardUsing the initial mass 1.510 g and the molecular formula of the hydrate CuCl2⋅2H2O). Predict the expected mass of water that should be released if heated.arrow_forwardchloric acid + barium hydroxide → barium chlorate + waterWhen 1.9 × 1022 particles of water are produced, 2.7 grams of barium hydroxide were reacted. What is the percent yield of this reaction?arrow_forward
- A 0.206 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid magnesium oxide. In the laboratory a student weighs the mass of the magnesium oxide collected from this reaction as 0.254 g. What is the percent yield of this reaction?arrow_forward5 g of hydrated barium chloride is heated in a crucible until the mass of the sample no longer changes. The mass of the sample after heating is 4.26 g. Assume that the mass lost during the heating is solely due to the loss of water from the sample. What percentage of water was contained in the barium chloride hydrate?arrow_forwardOne technique used in industry to extract gold from gold sulfide is reacting it with hydrogen gas. In the process, solid gold and hydrogen sulfide gas form. If 337.75 g of gold(III) sulfide is completely reacted in the process, what mass of gold will be produced?arrow_forward
- If 9.9 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂ that is produced?arrow_forwardChromium metal can be produced from high-temperature reactions of chromium (III) oxide with liquid silicon. The products of this reaction are chromium metal and silicon dioxide. If 8.21 grams of chromium (III) oxide and 4.11 grams of Si are combined, determine the total mass of reactants that are left over.arrow_forwardA student begins an experiment with 0.4631 g sample of aluminum can. At the start of week 2 the student determines that 5.0785 g of potassium alum,KAl(SO4)2•12H2O, were synthesized. What percent yield should the student report? Assuming that the aluminum is limiting.arrow_forward
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