4Ht +2NO3+ 2e-+2NO z+ZH2OCu +2NO2-t4Ht > cu+2NO2+ 2HZOHzO):Cucaqst ZNO3 caq) +4HgO Lagy o CueCags+2NO2(ags+6HThe chemical formula of "Product A" inCuz+cag>the net ionic equation is:c. In the space below, show the calculations that clearly identify the limiting reagent and writethe formula of the limiting reagent in the blank. Note that you will need to use your balanced netionic equation from above and the fact that you used 25.0 mL of 6.0 M HNO3 (nitric acid) andabout 1.00 g of copper.ImolcuO.9 Sg Cu (. Co = 0.0149 moles cu3.55g CuThe limiting reagent(reactant) is:July 16, 2018page 4-6

Solution stoichiometry is mainly based on the calculation of moles and volumes. These two values are…

Answered: 4Ht +2NO3+ 2e-+2NO z+ZH2O Cu +2NO2-t4Ht…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter11: Stoichiometry

Section: Chapter Questions

Problem 71A

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A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?
he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.
Many over-the-counter antacid tablets are now formulated using calcium carbonate as die active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting die stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a burp). Write die balanced chemical equation for this process.
The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry textbook estimates that if 1.00 × 108 tons Mg were taken out of the sea each year, it would take one million years for the Mg concentration to drop to 0.12%. Do sufficient calculations to either verify or refute this statement. Assume that Earth is a sphere with a diameter of 8000 mi, 67% of which is covered by oceans to a depth of 1 mi, and that no Mg is washed back into the oceans at any time.
What is true about the chemical properties of the product? a. The properties are more like chemical A. b. The properties are more like chemical B. c. The properties are an average of those of chemical A and chemical B. d. The properties are not necessarily like either chemical A or chemical B. e. The properties arc more like chemical A or more like chemical B, but more information is needed. Justify your choice, and for choices you did not pick, explain what is wrong with them.
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
The meat from one hazelnut has a mass of 0.985 g. (a) What is the mass of a millionth of a mole (106) of hazelnut meats? (A millionth of a mole is also called a micromole.) (b) How many moles are in a pound of hazelnut meats?
It sodium peroxide is added to water, elemental oxygen gas is generated: :math>Na2O2(s)+H2O(l)NaOH(aq)+O2(g) ppose 3.25 g of sodium peroxide is added to a large excess of water. What mass of oxygen gas will be produced?
Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and 25C, it has a density of 1.71 g/L. (a) What is the molar mass of cyclopropane? (b) Cyclopropane is made up of 85.7% C and 14.3% H. What is the molecular formula of cyclopropane?
When yeast is added to a solution of glucose or fructose, the sugars are said to undergo fermentation, and ethyl alcohol is produced. :math>C6H12O6(aq)2C2H5OH(aq)+2CO2(g) is is the reaction by which wines arc produced from grape juice. Calculate the mass of ethyl alcohol, C2H5OH. Produced when 5.25 g of glucose, C6H12O6, undergoes this reaction.
Alum [KAl(SO₄)₂.xH2O] is used in food preparation, dyefixation, and water purification. To prepare alum, aluminum isreacted with potassium hydroxide and the product with sulfuricacid. Upon cooling, alum crystallizes from the solution.(a) A 0.5404-g sample of alum is heated to drive off the watersof hydration, and the resulting KAl(SO₄)₂weighs 0.2941 g. De-termine the value of xand the complete formula of alum.(b) When 0.7500 g of aluminum is used, 8.500 g of alum forms.What is the percent yield?

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