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Interpretation:
The limiting reactant when
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EBK INTRODUCTORY CHEMISTRY
- Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide. Starting with 2.2 mol NO, calculate how many moles and how many grams of O2 are required for complete reaction. Calculate what mass of NO2, in grams, is produced.arrow_forwardUrea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. (NH2)2CO(s) + H2O() 2 NH3(aq) + CO2(g) (a) When 300. g urea and 100. g water are combined, calculate the mass of ammonia and the mass of carbon dioxide that form. (b) Calculate the mass of the excess reactant that remains after reaction.arrow_forwardYou react nitrogen and hydrogen in a container to produce ammonia, NH3(g). The following figure depicts the contents of the container after the reaction is complete. a Write a balanced chemical equation for the reaction. b What is the limiting reactant? c How many molecules of the limiting reactant would you need to add to the container in order to have a complete reaction (convert all reactants to products)?arrow_forward
- Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.arrow_forwardA potential fuel for rockets is a combination of B5H9 and 0 2. The two react according to the following balanced equation: 2B5H9(l)+12O2(g)5B2O3(s)+9H2O(g) If one tank in a rocket holds 126 g B5H9 and another tank holds 192 g O2, what mass of water can be produced when the entire contents of each tank react together?arrow_forward4.12 In petroleum refining, hydrocarbons are often manipulated by reacting them with H2(g). If hexene, C6H12, is reacted with hydrogen to form hexane, C6H14, how many moles of hydrogen are needed to react with 453 moles of hexene?arrow_forward
- 4.27 Copper reacts with sulfuric acid according to the following equation: 2H2SO4+CuCuSO4+2H2O+SO2 How many grams of sulfur dioxide are created by this reaction if 14.2 g of copper reacts with 18.0 g of sulfuric acid?arrow_forwardThe compound SF6 is made by burning sulfur in an atmosphere of fluorine. The balanced equation is Sa(s) + 24 F2(g) SF6(g) Starting with a mixture of 1.6 mol of sulfur. Sg, and 35 mol of F2, (a) Which is the limiting reagent? (b) What amount of SF6 is produced?arrow_forward4.24 Ammonia gas can be prepared by the reaction CaO(s)+2NH4Cl(s)2NH3(g)+H2O(g)+CaCl2(s) If 112 g of CaO reacts with 224 g of NH4Cl, how many moles of reactants and products are there when the reaction is complete?arrow_forward
- The principal constituent of natural gas is methane, which burns in air according to the reaction CH4+2O2CO2+2H2O How many grams of O2 are needed to produce 3.50 g of CO2?arrow_forwardAluminum chloride, Al2Cl6, is an inexpensive reagent used in many industrial processes. It is made by treating scrap aluminum with chlorine according to the balanced equation 2 Al(s) + 3 Cl2(g) Al2Cl6(S) (a) Determine which reactant is limiting if 2.70 g Al and 4.05 g Cl2 are mixed. (b) Calculate what mass of Al2Cl6 can be produced. (c) Calculate what mass of the excess reactant remains when the reaction is complete.arrow_forwardAqueous solutions of iron(II) chloride and sodium sulfide react to form iron(II)sulfide and sodium chloride. (a) Write the balanced equation for the reaction. (b) If you combine 40. g each of Na2S and FeCl2, what is the limiting reactant? (c) What mass of FeS is produced? (d) What mass of Na2S or FeCl2 remains after the reaction? (e) What mass of FeCl2 is required to react completely with 40. g of Na2S?arrow_forward
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