Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid. How many total moles of acid (moles of HCl and H3PO4 combined) are formed when starting with 4.5 g of PCI5 and excess H2O? PCI5 + 4H20 → 5HCI + H3PO4 0.12 moles O 0.13 moles O 27 moles O 23 moles O 0.022 moles

Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid. How many total moles of acid (moles of HCl and H3PO4 combined) are formed when starting with 4.5 g of PCI5 and excess H2O? PCI5 + 4H20 → 5HCI + H3PO4 0.12 moles O 0.13 moles O 27 moles O 23 moles O 0.022 moles

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter6: Chemical Calculations: Formula Masses, Moles, And Chemical Equations

Section: Chapter Questions

Problem 6.61EP: For the chemical reaction Sb2S3+6HCl2SbCl3+3H2S write the conversion factor that would be needed to...

See similar textbooks

Similar questions

One mol of ammonia reacts with 1.00 mol of oxygen to form nitrogen oxide and water according to the reaction 4NH3(g)+5O2(g)4NO(g)+6H2O(l)State which statements are true about the reaction and make the false statements true. (a) All the oxygen is consumed. (b) 4.00 mol NO are produced. (c) 1.50 mol H2O are produced. (d) The description of the experiment does not provide enough information to determine percent yield. (e) Three moles of water are produced for every two moles of NO obtained.
For each of the following incomplete and unbalanced equations, indicate how many moles of the second reactant would be required to react completely with 0. 145 mole of the first reactant. msp;BaCl2(aq)+H2SO4(aq) msp;AgNO3(aq)+NaCl(aq) msp;Pb(NO3)2(aq)+Na2CO3(aq) msp;C3H8(g)+O2(g)
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%.
3.59 The composition of materials such as alloys can be described in terms of mole percentage (mol%), atom percentage (at%), or weight percentage (wt%). Carry out the following conversions among these units. (a) 60 Cu and 40 Al to at%, (b) 25 mol% NiO and 75 mol % MgO to wt%, (C) 40 wt% MgO and 60 wt% Feo to mol %
For the chemical reaction Sb2S3+6HCl2SbCl3+3H2S write the conversion factor that would be needed to do each of the following one-step conversions. a. Moles of SbCl3 to moles of H2S b. Moles of Sb2S3 to moles of HCl c. Moles of H2S to moles of HCl d. Moles of Sb2S3 to moles of SbCl3
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.
3.11 Balance the following equations. (a) CaC2(s) + H2O(l)( Ca(OH)2(s) + C2H2(g) (b) (NH4)2CrO7(s) ( Cr2O3(s) + N2(g) + H2O (g) (c) CH3NH2(g) + O2(g) ( CO2(g) + N2(g) + H2O (g)
Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form carbon tetrafluoride and nitrogen trifluoride. C2N2(g)+7F2(g)2CF4(g)+2NF3(g)(a) How many moles of fluorine react with 1.37 mol of cyanogen? (b) How many moles of CF4 are obtained from 13.75 mol of fluorine? (c) How many moles of cyanogen are required to produce 0.8974 mol of NF3? (d) How many moles of fluorine will yield 4.981 mol of nitrogen trifluoride?
4.23 In the reaction of arsenic with bromine, AsBr5 will form only when excess bromine is present. Write a balanced chemical equation for this reaction. Determine the minimum number of motes of bromine that are needed if 9.6 moles of arsenic is present.
For the following reactions, write the ratios that can be established among molar amounts of the various compounds. 2H2+O22H2O 2H2O22H2O+O2 P4+5O2P4O10 2KClO32KCl+3O2 xs