DATA: weight of the crucible + lid (Worucible-Hid) =30.4265 weight of the crucible + lid + magnesium (Worucible lid+Mg) =30.6831 weight of the product + crucible + lid (Worucible-Hlid-Mgo) =30.7168 mass of the product (mg0) = ? CALCULATIONS: Mass of magnesium: mMg = Mass of oxygen: mo = Number of moles of Mg: Mg = Number of moles of O: no = Mole ratio of Mg to O in the compound: Mg / no = Empirical (simplest) formula of the compound: Molecular formula of the compound (Note that the compound is an ionic compound) |

DATA: weight of the crucible + lid (Worucible-Hid) =30.4265 weight of the crucible + lid + magnesium (Worucible lid+Mg) =30.6831 weight of the product + crucible + lid (Worucible-Hlid-Mgo) =30.7168 mass of the product (mg0) = ? CALCULATIONS: Mass of magnesium: mMg = Mass of oxygen: mo = Number of moles of Mg: Mg = Number of moles of O: no = Mole ratio of Mg to O in the compound: Mg / no = Empirical (simplest) formula of the compound: Molecular formula of the compound (Note that the compound is an ionic compound) |

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 25QAP: Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and...

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Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and 25C, it has a density of 1.71 g/L. (a) What is the molar mass of cyclopropane? (b) Cyclopropane is made up of 85.7% C and 14.3% H. What is the molecular formula of cyclopropane?
Use the web to determine the differences in the amounts of aluminum recycled in states where there are deposits on aluminum cans versus states where recycling is voluntary. What is the most reliable way to estimate this value? mat uncertainty is there in the estimate?
Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.
TheoreticalYield=57.1g Actual=23.9g % Yield = ____________
DATA: weight of the crucible + lid (Worucible Hid) =30.4265 weight of the crucible + lid + magnesium (Worucibletlid+Mg) =30.6831 weight of the product + crucible + id (Werucible-tid+Mg 0) =30.7168 mass of the product (mmgo) = ?/ CALCULATIONS: Mass of magnesium: mMg = Mass of oxygen: mo = Number of moles of Mg: Number of moles of O: no = Mole ratio of Mg to O in the compound: Mg / no = Empirical (simplest) formula of the compound:
Given the following set of data for the determination of empirical formula of magnesium oxide: - Mass of empty crucible = 15.79 g - Mass of crucible + magnesium = 16.43 g - Mass of crucible + magnesium oxide = 16.79 g - Molar mass (g/mol): Mg = 24.4; 0 = 16.0 The molar ratio of Mg to O is 0.86 APIT OF ENGINEERING 0.79 1.27 1.17 0.95
An organic liquid is either methyl alcoholethyl alcohol or a mixture of the two.A 0.220 g sample of the liquid is burned in an excessof and yields 0.352 g Is the liquid apure alcohol or a mixture of the two?
Part A Copper atoms are heavier than magnesium atoms. So, although each atom of magnesium can produce one atom of copper, the masses won't be the same. The ratio of the atomic weight of copper to the atomic weight of magnesium is about 2.61. Given this ratio and the initial mass of the magnesium strip measured in task 1, part A, calculate the mass of copper that can be produced. Recall: Mg + Cu(NO3)2 Mg(NO3)2 Cu + В I x' X, Font Sizes E E Characters used: 0/ 15000 Part B In this step, you'll reduce the solution in test tube 4 and extract the copper solids. Read ahead so you VO 11:3 III !!
15. Laboratory analysis of a sample yielded the following data for the combustion of Nickel Ni(s) + O2(g) àNi O(s) i) Mass of a crucible = 30.02g ii) Mass of nickel (Ni) and crucible = 31.07 g iii) Mass of nickel oxide and crucible = 31.36 g Based on the above information, calculate the following iv) Mass of nickel (Ni) in sample = v) Mass of nickel oxide = c) Based on the above calculate the Theoretical Yield of Nickel oxide obtained from the mass of nickel in part (iv) above d) Calculate the percentage yield of nickel oxide
Mass of Na2CO3.H2O (g) = 2.12g (g) Mass of the CaCl2.2H2O (g) = 1.98g Mass of the top funnel + filter paper (g) = 15.85g Mass of top funnel + filter paper + CaCO3 collected (g) = 17.81g CaCl2 + Na2CO3 ==== CaCo3 + 2NaCl Moles Na2CO3 reacting? Moles CaCO3 reacting? Moles CaCO3 produced by the LR? Theoretical yield in moles and grams? Reagent in excess? Moles of reagent in excess left unreacted? Mass of precipitate? Experimental yield? Percent yield?
Valuable minerals (chemicals) can be obtained from ores, which are natually occuring mixtures. One ore cotains 38% magnetite, a mineral with the chemical formual Fe3O4. Fe3O4 contains 72.4% iron. What mass of ore (in tons) would contain 3.5 tons of iron? (Hint: your mass percent conversion factors can have units of tons) *Mass percent values used in calculations should be written as conversion factors with units & labels
Mass of Na2CO3.H2O (g) = 2.12g (g) Mass of the CaCl2.2H2O (g) = 1.98g Mass of the top funnel + filter paper (g) = 15.85g Mass of top funnel + filter paper + CaCO3 collected (g) = 17.81g CaCl2 + Na2CO3 ==== CaCo3 + 2NaCl Moles CaCO3 produced by Na2CO3 (if all Na2CO3 reacts)? Moles CaCO3 produced by Na2CO3 (if all CaCl2 reacts)? What is the Limiting Reagent? Moles Na2CO3 reacting? Moles CaCl2 reacting?