3. If at S.T.P 4.48 L of NH3(g) is allowed to react with 9.03 x 1022 molecules of O₂(g), please answer the questions for the following reaction: 4NH3(g) + 5O2(g) a. What is the limiting reactant? Please show all your work. - b. What mass of nitrogen monoxide can be expected? 6H₂O(g) + 4NO(g) c. If 3.00 g of nitrogen monoxide recovered, what would the percentage yield be? d. What reactant is in excess? Following the reaction, what is the remaining mass of the excess reactant?

3. If at S.T.P 4.48 L of NH3(g) is allowed to react with 9.03 x 1022 molecules of O₂(g), please answer the questions for the following reaction: 4NH3(g) + 5O2(g) a. What is the limiting reactant? Please show all your work. - b. What mass of nitrogen monoxide can be expected? 6H₂O(g) + 4NO(g) c. If 3.00 g of nitrogen monoxide recovered, what would the percentage yield be? d. What reactant is in excess? Following the reaction, what is the remaining mass of the excess reactant?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 164CP: Nitric acid is produced commercially by the Ostwald process, represented by the following equations:...

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Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.
When solid silicon tetrachloride reacts with water, solid silicon dioxide and hydrogen chloride gas are formed. (a) Write a balanced equation for the reaction. (b) In an experiment, 45.00 g of silicon tetrachloride are treated with 45.00 mL of water (d=1.00g/mL). What is the theoretical yield of HCI (in grams)? (c) When the reaction is complete, 17.8 L of HCl gas (d=1.49g/L at the conditions of the experiment) are obtained. What is the percent yield? (d) How much of the reactant in excess is unused?
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
The space shuttle environmental control system handles excess CO2 (which the astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle, and each exhales 20. L of air pee minute, how long could clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 g/mL.
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
4.90 Iron metal can be refined (rom the mineral hematite (Fe2O3). One way of converting the mineral to iron is to react it with carbon monoxide, as shown below: Fe2O3+3CO2Fe+3CO2 Because the hematite is obtained from various ores, it is usually not in a pure form. Suppose an iron manufacturer has 2.00 X 105 kg of ore available, and the ore is 93% Fe2O3 by mass. (There is no iron in the remaining 7% of the ore.) How many moles of Fe2O3are present in this ore? How many kg of pure iron could be obtained from this sample of ore? Assume that the process has a 100% yield and that excess CO is available.
4.19 How many metric tons of carbon are required to react with 7.83 metric tons of Fe2O3 according to the following reaction? 2Fe2O3+3C3CO2+4Fe How many metric tons of iron are produced?
Propane, C3H8, is the fuel of choice in a gas barbecue. When burning, the balanced equation is C3H8+5O23CO2+4H2O a What is the limiting reactant in cooking with a gas grill? b If the grill will not light and you know that you have an ample flow of propane to the burner, what is the limiting reactant? c When using a gas grill you can sometimes turn the gas up to the point at which the flame becomes yellow and smokey. In terms of the chemical reaction, what is happening?
Bacterial digestion is an economical method of sewage treatment. The reaction is an intermediate step in the conversion of the nitrogen in organic compounds into nitrate ions. What mass of bacterial tissue is produced in a treatment plant for every 1.0 104 kg of wastewater containing 3.0% NH4+ ions by mass? Assume that 95% of the ammonium ions are consumed by the bacteria.