LIMITING REAGENTS TO2/S12 Based on the balanced equation Molar Mass (g/mol) 2C4Н10 + 1302 - 8СО2 + 10Н20 C4H10 calculate the number of excess reagent units remaining when 142 CaH10 molecules and 871 0, molecules react? 58.124 32.000 Co2 Н20 Avogadro's No. 6.022x1023 mol1 44.010 18.015 exact number, no tolerance Question Attempts: 0 of 1 used SUBMIT ANSWER SAVE FOR LATER

LIMITING REAGENTS TO2/S12 Based on the balanced equation Molar Mass (g/mol) 2C4Н10 + 1302 - 8СО2 + 10Н20 C4H10 calculate the number of excess reagent units remaining when 142 CaH10 molecules and 871 0, molecules react? 58.124 32.000 Co2 Н20 Avogadro's No. 6.022x1023 mol1 44.010 18.015 exact number, no tolerance Question Attempts: 0 of 1 used SUBMIT ANSWER SAVE FOR LATER

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 30A

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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.
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.
Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
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.
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)
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onsider the balanced chemical equation :math>4Al(s)+3O2(g)2Al2O3(s). at mole ratio would you use to calculate how many moles of oxygen gas would be needed to react completely with a given number of moles of aluminum metal? What mole ratio would you use to calculate the number of moles of product that would be expected if a given number of moles of aluminum metal reacts completely?
4-89 If 7.0 kg of is added to 11.0 kg of to form which reactant is in excess?
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.
How many molecules of the sweetener saccharin can be prepared from 30 C atoms, 25 H atoms, 12 0 atoms, 8 S atoms, and 14 N atoms?
Nitrogen (N2) and hydrogen (H2)react to form ammonia (NH3). Consider the mixture of N2 and H2 in a closed container as illustrated below: Assuming the reaction goes to completion, draw a representation of the product mixture. Explain how you arrived at this representation.
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