Section 5.9 The Mole and Chemical Equations 11. In the following equations consider the bold formulas. The molar ratio between the two bold formulas can be expressed in two ways. Write them both. a. S(s) + O2(g) → SO2(g) b. Sr(s) +2H2O(1) → Sr(OH)2(s) + H2(g) c. 4NH3(g) +5O2(g) → 4NO(g) + 6H2O(g) d. CaO(s) + 3C(s) → CaC2(s) +CO(g)

Section 5.9 The Mole and Chemical Equations 11. In the following equations consider the bold formulas. The molar ratio between the two bold formulas can be expressed in two ways. Write them both. a. S(s) + O2(g) → SO2(g) b. Sr(s) +2H2O(1) → Sr(OH)2(s) + H2(g) c. 4NH3(g) +5O2(g) → 4NO(g) + 6H2O(g) d. CaO(s) + 3C(s) → CaC2(s) +CO(g)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 124E: DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a...

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The gaseous hydrocarbon acetylene, C2H2, is used in welders’ torches because of the large amount of heat released when acetylene burns with oxygen. :math>2C2H2(g)+5O2(g)4CO2(g)+2H2O(g) w many grams of oxygen gas are needed for the complete combustion of 150 g of acetylene?
The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A at-oms are shown in blue and B atoms in white). The box on the left represents the box on the right shows what is left once the reaction has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Consider the balanced chemical equation :math>A+5B3C+4D en equal masses of A and B are reacted, which is limiting, A or B? Justify your choice. If the molar mass of A is greater than the molar mass of B, then A must be limiting. If the molar mass of A is less than the molar mass of B, then A must be limiting. If the molar mass of A is greater than the molar mass of B, then B must be limiting. If the molar mass of A is less than the molar mass of B, then B must be limiting.
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients.
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.
4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
If baking soda (sodium hydrogen carbonate) is heated strongly, the following reaction occurs: :math>2NaHCO3(s)Na2CO3(s)+H2O(g)+CO2(g) lculate the mass of sodium carbonate that will remain if a 1.52-g sample of sodium hydrogen carbonate is heated.
The active ingredient in aspirin is acetylsalicylic acid, which has the chemical formula C9H8O4. An aspirin pill contains 300.0 mg of acetylsalicylic acid. How many moles of acetylsalicylic acid does it contain?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
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itamin B12 , cyancobalamin, is essential for human nutrition. Its molecular formula is C63H88CoN14O14P . A lack of this vita min in the diet can lead to anemia. Cyanocohalamin is the form of the vitamin found in vitamin supplements. l type='a'> What is the molar mass of cyanocobalamin to two decimal places? How many moles of cyanocohalamin molecules are present in 250 mg of cyanocobalamin? What is the mass of 0.60 mole of cyanocobalamin? How many atoms of hydrogen are in 1 .0 mole of cyanocobalamin? What is the mass of 1.0107 molecules of cyanocobalamin? What is the mass (in grams) of one molecule of cyanocobalamin?