LIMITING REAGENTS T02/S12 Based on the balanced equation Molar Mass (g/mol) CaH2 + 2H20 - Ca(OH)2 + 2H2 СаН2 Н2о Ca(ОН)2 Н2 Avogadro's No. 6.022x1023 mol"1 42.094 calculate the number of excess reagent units remaining when 90 CaH2 formula units and 188 H20 molecules react? 18.015 74.092 2.016 exact number, no tolerance

LIMITING REAGENTS T02/S12 Based on the balanced equation Molar Mass (g/mol) CaH2 + 2H20 - Ca(OH)2 + 2H2 СаН2 Н2о Ca(ОН)2 Н2 Avogadro's No. 6.022x1023 mol"1 42.094 calculate the number of excess reagent units remaining when 90 CaH2 formula units and 188 H20 molecules react? 18.015 74.092 2.016 exact number, no tolerance

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter11: Stoichiometry

Section: Chapter Questions

Problem 5STP

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A dark brown binary compound contains oxygen and ametal. It is 13.38% oxygen by mass. Heating it moderatelydrives off some of the oxygen and gives a red binary compoundthat is 9.334% oxygen by mass. Strong heatingdrives off more oxygen and gives still another binary compound,which is only 7.168% oxygen by mass. (a) Compute the mass of oxygen that is combined with1.000 g of the metal in each of these three oxides. (b) Assume that the empirical formula of the first compoundis MO2 (where M representsthe metal). Givethe empirical formulas of the second and thirdcompounds. (c) Name the metal.
C6H8O7 (aq) + 3 NaHCO3 (aq) → 3 CO2 (g) + 3 H2O (l) + Na3C6H5O7 (aq) Based on the above equation, how do I use the amount/volume of CO2 produced to determine the percent composition of citric acid and sodium bicarbonate in Alka Seltzer? Here are the instructions: C6H8O7 (aq) + 3 NaHCO3 (aq) → 3 CO2 (g) + 3 H2O (l) + Na3C6H5O7 (aq) Use the Ideal Gas Law to determine the amount of collected CO2 Use that quantity to determine the percent composition of citric acid and the percent composition of sodium bicarbonate in Alka Seltzer. They do not need to add up to 100% because there are other ingredients in Alka Seltzer.
Aniline (C6H5NH2) can be produced from chlorobenzene (C6H5Cl) via the following reaction: C6H5Cl (l) + 2 NH3 (g) ⟶ C6H5NH2 (l) + NH4Cl (s) Assume that 20.0 g of chlorobenzene at 92% purity is mixed with 8.30 g of ammonia. a) Which is the limiting reactant? b) Which reactant is present in excess? c) What is the theoretical yield of ammonium chloride in grams? d) If 4.78 g of NH4Cl was recovered, what was the percent yield? e) How many grams of a the limiting reagent must be used to isolate 10.20 g of C6H5NH2? Assume this is a separate experiment than the one described above. Also assume a purity of 92% for chlorobenzene and the same percent yield.
3.Use the following Unbalanced reaction and the information about starting material to determine the limiting reagent and find the maximum mass of the product in question. Na2CO3 + CaCl2 --> CaCO3 + NaCl 44.3 g Na2CO3 and 73.7 g CaCl2 are reacted. What is the max NaCl produced?
3. Use the following Unbalanced reaction and the information about starting material to determine the limiting reagent and find the maximum mass of the product in question. Na2CO3 + CaCl2 --> CaCO3 + NaCl 44.3 g Na2CO3 and 73.7 g CaCl2 are reacted. What is the max NaCl produced?
plant photosynthesis sugars and oxygen from carbon dioxide and water are shown 6co2+6h2o=c6h12o6+o6 calculate %yield of 1.24g of c6h12o6 are produced by reaction of 1.24of cp2. the molar mass is 44.01g and the molar mass of c6h12o6 is 180.2g
Citric acid (C6 H8 O7) named for its natural occurrence in citrus fruits, is produced in large quantities industrially. This is often achieved through large-scale fermentation of sucrose and/or glucose. The reaction involving sucrose is summarized below: C12 H22 O11 + 3O2 ------> 2C6 H8 O7 + 3H2O How many grams of citric acid would be produced from 700.0 kg of sucrose assuming a percent yield of 93.10%
H3PO4 + 3NaOH ---> Na3PO4 + 3H2O If you mix 100 ml of 8.5M H3PO4 with 150 ml of 9.0M NaOH, how many g of Na3PO4 will be produced? What is your limiting reagent? If you only got 59.5 g of Na3PO4, what is your percent yield? How many grams of your excess reagent do you have left over?
Given the following balanced reaction 4KNO3 (aq) → 2K2O (s) + 2N2 (g) + 5O2 (g), fill in the blanks for the road maps for the following situations: a) Moles of O2 produced from the decomposition of moles of KNO3. b) Mass of N2 produced when moles of K2O is produced. c) Mass of KNO3 decomposed when grams of K2O is produced. Can only use this to answer the question mole of kno3, mqass of kno3, molar ration, molar mass, moles o2, mole n2, mass n2, mass k20, mole k20
Dteremine the limiting reaganet (SHOW THE calculations for determinig the limiting reagent ) and calculate the theoretical mass of PbI2 by using limiting reagent. show your calculations. Balanced Equation: Pb(NO3)2 (aq) + 2KCL(aq) ---> 2KNO3(aq) + PbI2(s) No of moles of Pb(NO3)2 = 0.003 No of moles of KI = 0.007
Use stoichiometry (Ch 13) to calculate how many grams of PbSO4(s) would be produced if 5.50 grams of LiNO3 were produced. It will be helpful to do this on paper first. Li2SO4(aq) + Pb(NO3)2(aq) ⟶2 LiNO3(aq) + PbSO4(s) a. Select the value for the molar mass of LiNO3, with the correct value, significant figures, and units. b. Select the value for the molar mass of PbSO4, with the correct value, significant figures, and units. c. Select the mole ratio that will be used, with the correct values and units. d. Select the first operation and conversion factor used to cancel the given unit and substance. e. Lastly, select the calculated answer, expressed with the appropriate significant figures and unit.
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3NH3 to NONO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g)4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 1.25 gg of NH3NH3 reacts with 1.75 g of O2O2. question: How many grams of the excess reactant remain after the limiting reactant is completely consumed? Express your answer in grams to three significant figures