What mass in grams of nitric acid is required to react with 240 g C;H,?Express your answer with the appropriate units.Toluene (C;Hs) and nitric acid (HNO,) are used inthe production of trinitrotoluene (TNT,C;HsN3Os), an explosive.CHs + HNO-C;H;N3O6+ H20 (notbalanced)mass of nitric acidValueUnitsSubmitRequest AnswerPart BWhat mass in grams of TNT can be made from 646 g C;Hs?Express your answer with the appropriate units.mass of TNT-ValueUnitsSubmitRequest Answer

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What mass in grams of nitric acid is required to react with 240 g C;H,? Express your answer with the appropriate units. Toluene (C;Hs) and nitric acid (HNO,) are used in the production of trinitrotoluene (TNT, CHsN3Os), an explosive. CHs + HNO-C;H&N3O+H20 (not balanced) mass of nitric acid Value Units Submit Request Answer • Part B What mass in grams of TNT can be made from 646 g CHa? Express your answer with the appropriate units. mass of TNT- Value Units Submit Request Answer

What mass in grams of nitric acid is required to react with 240 g C;H,? Express your answer with the appropriate units. Toluene (C;Hs) and nitric acid (HNO,) are used in the production of trinitrotoluene (TNT, CHsN3Os), an explosive. CHs + HNO-C;H&N3O+H20 (not balanced) mass of nitric acid Value Units Submit Request Answer • Part B What mass in grams of TNT can be made from 646 g CHa? Express your answer with the appropriate units. mass of TNT- Value Units Submit Request Answer

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 20CR: Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous...

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Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. l type='a'> Write the balanced equation for the reaction that is (occurring. including all phases. If a 100.0-g sample of calcium carbide (CaC2)is initially reacted with 50.0 g of water, which reactant is limiting? Prove that mass is conserved for the reactant amounts used in pan b.
Sodium borate decahydrate, Na2B4O710H2O is commonly known as borax. It is used as a deodorizer and mold inhibitor. A sample weighing 15.86 g is heated until a constant mass is obtained indicating that all the water has been evaporated off. (a) What percent, by mass of Na2B4O710H2O is water? (b) What is the mass of the anhydrous sodium borate, Na2B4O7?
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
A mordant is a substance that combines with a dye to produce a stable fixed color in a dyed fabric. Calcium acetate is used as a mordant. It is prepared by the reaction of acetic acid with calcium hydroxide. 2CH3CO2H+Ca(OH)2Ca( CH3 CO2)2+2H2O What mass of Ca(OH)2 is required to react with the acetic acid in 25.0 mL of a solution having a density of 1.065 g/mL and containing 58.0% acetic acid by mass?
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
When 9.59 g of a certain vanadium oxide is heated in the presence of hydrogen, and a new oxide of vanadium are formed. This new vanadium oxide has a mass of 8.76 g. When the second vanadium oxide undergoes additional heating in the presence Of hydrogen, 5.38 g of vanadium metal forms, a. Determine the empirical formulas for the two vanadium oxides. b. Write balanced equations for the Steps of the reaction. c. Determine the mass of hydrogen needed to complete the steps of this reaction.
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?
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
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. D 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.
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.
Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.