When perchloric acid (HCIO4) reacts with tetraphosphorus decaoxide, phosphoric acid and dichlorine heptaoxide are produced. The balanced equation for this reaction is: 12HCIO4 (aq) + P4010 (s) 4H3PO04 (aq) + 6Cl,0, (1) If 2 moles of tetraphosphorus decaoxide react, The reaction consumes moles of perchloric acid (HCIO4) The reaction produces moles of phosphoric acid and moles of dichlorine heptaoxide

When perchloric acid (HCIO4) reacts with tetraphosphorus decaoxide, phosphoric acid and dichlorine heptaoxide are produced. The balanced equation for this reaction is: 12HCIO4 (aq) + P4010 (s) 4H3PO04 (aq) + 6Cl,0, (1) If 2 moles of tetraphosphorus decaoxide react, The reaction consumes moles of perchloric acid (HCIO4) The reaction produces moles of phosphoric acid and moles of dichlorine heptaoxide

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 3CR

See similar textbooks

Similar questions

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.
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%.
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.
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?
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.
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.
In a winter country, a winemaker is waiting for her grapes to freeze in order to make a special batch of holiday ice wine. Recent analysis has shown that the grapes are currently 30% glucose by mass. Assume that glucose (formula C6H12O6 MW= 180 g/mol) is the only solute present and that water is the solvent. Use Kfwater = 1,86°C kg/mol. What is the mass of glucose present? How many moles of glucose are there (three significant figures)? What is the mass of water present (in grams)? (Hint: Solution - Solute = Solvent) What is the molality of sucrose in water? What is the freezing point of the grapes (deg C)? What is the freezing point (deg C) if the molality of the glucose in water is 2.16 mol/kg?
A 13.2010g sample of hydrated zinc sulfate, ZnSO4 • xH2O), was strongly heated until no further change in mass was recorded. The final mass of solid product was found to be 7.3997g. On heating, all of the water of crystallization had evaporated, as shown by the equation: ZnSO4 • xH2O -> ZnSO4 + xH2O Calculate the number of moles of water of crystallization in the sample. Write in a padpaper and show the complete solution
A 13.2010g sample of hydrated zinc sulfate, ZnSO4 • xH2O), was strongly heated until no further change in mass was recorded. The final mass of solid product was found to be 7.3997g. On heating, all of the water of crystallization had evaporated, as shown by the equation: ZnSO4 • xH2O -> ZnSO4 + xH2O Calculate the number of moles of water of crystallization in the sample. Write clearly and show the complete solution
Imagine that you are given 0.2500 g of a sample of copper(II) sulfate pentahydrate (CuSO4 • 5 H2O). You very carefully heat the compound for an extended period of time to drive off water, after which you determine the mass of the remaining solid to be 0.1598 g. Determine whether the data given confirm the formula of the hydrate. You must show any relevant calculation
GivenRaw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfurWhereas the balanced chemical reaction, as given in the problem is: CaS5+2HCl => 4S + CaCl2 + H2Sa. Find the Mass to Mass Stoichiometry Calculation b. Upon solving A, find the LIMITING REAGENT, EXCESS REAGENT and the AMOUNT IN EXCESSc. Find the Percentage Yield from Problem A
How many grams of P2O5P2O5 are formed when 9.51 g 9.51 g of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots.