LIMITING REAGENTS T02/s22 Based on the balanced equation Molar Mass (g/mol) 2NBr3 + 3NaOH - N2 + 3NaBr + 3HOBR NB33 253.72 calculate the number of of excess reagent units remaining when 160 NBr3 molecules and 270 NaOH formula units react? 39.997 NaOH N2 NaBr 28.013 102,800 НOBr 96.911 Avogadro's No. 6.022x1023 mol"1 exact number, no tolerance LIMITING REAGENTS T02/S12 Based on the balanced equation Molar Mass (g/mol) СаHz + 2H20 - Сa(ОН)2 + 2H2 Cан2 Н2о Cа(ОН)2 На Avogadro's No. 6.022x1023 mol1 42.094 calculate the number of excess reagent units remaining when 38 CaH, formula units and 68 H20 molecules react? 18.015 74.092 2.016 exact number, no tolerance

LIMITING REAGENTS T02/s22 Based on the balanced equation Molar Mass (g/mol) 2NBr3 + 3NaOH - N2 + 3NaBr + 3HOBR NB33 253.72 calculate the number of of excess reagent units remaining when 160 NBr3 molecules and 270 NaOH formula units react? 39.997 NaOH N2 NaBr 28.013 102,800 НOBr 96.911 Avogadro's No. 6.022x1023 mol"1 exact number, no tolerance LIMITING REAGENTS T02/S12 Based on the balanced equation Molar Mass (g/mol) СаHz + 2H20 - Сa(ОН)2 + 2H2 Cан2 Н2о Cа(ОН)2 На Avogadro's No. 6.022x1023 mol1 42.094 calculate the number of excess reagent units remaining when 38 CaH, formula units and 68 H20 molecules react? 18.015 74.092 2.016 exact number, no tolerance

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 7ALQ

See similar textbooks

Similar questions

Chlorine and fluorine react to form gaseous chlorine trifluoride. Initially, 1.75 mol of chlorine and 3.68 mol of fluorine are combined. (Assume 100% yield for the reaction.) (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of chlorine trifluoride in moles? (d) How many moles of excess reactant remain after reaction is complete.
Air Pollution Nitrogen monoxide, which is present in urban air pollution, immediately Converts to nitrogen dioxide as it reacts with oxygen. a. Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen monoxide. b. What mole ratio would you use to convert from moles of nitrogen monoxide to moles of nitrogen dioxide?
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)
Titanium dioxide, TiO2 , reacts with carbon and chlorineto give gaseous TiCl4 : TiO2+2C+2Cl2TiCl4+2CO The reaction of 7.39 kg titanium dioxide with excess Cand Cl2 gives 14.24 kg titanium tetrachloride. Calculatethe theoretical yield of TiCl4 (assuming complete reaction)and its percentage yield.
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.
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?
Fertilizer The compound calcium cyanamide (CaNCN) is used as a nitrogen source for crops. To obtain this compound, calcium carbide is reacted with nitrogen at high temperatures. CaC2(s)+N2(g)CaNCN(s)+C(s) What mass of CaNCN can be produced if 7.50 mol of CaC2 reacts With 5.00 molOf N2 ?
For each of the following balanced chemical equations, calculate how many moles of product(s) would be produced if 0.500 mole of the first reactant were lo react completely. msp;CO2(g)+4H2(g)CH4(g)+2H2O(l) msp;BaCl2(aq)+2AgNO3(aq)2AgCl(s)+Ba(NO3)2(aq) msp;C3H8(g)+5O2(g)4H2O(l)+3CO2(g) msp;3H2SO4(aq)+2Fe(s)Fe2(SO4)3(aq)+3H2(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%.
Antacids Magnesium hydroxide is an ingredient in some antacids. Antacids react with excess hydrochloric acid in the stomach to relieve indigestion. Mg(OH)2+HClMgCl2+H2O a. Balance the reaction of Mg(OH)2 with HCI. b. Write the mole ratio that would be used to determine the number of moles of MgCl2 produced when HCI reacts with Mg(OH)2 .