Homework Answers
Answer 1. The burning magnesium ribbon produces light of sufficient intensity to cause temporary loss of sight. The burning ofmagnesium in air produces intense heat which can cause burns and initiate combustion in flammable materials and can be dangerous to our eyes too.
Answer 2.
1 mole of N = 2.5 mole of O
2 mole of N = 5 mole of O
Therefore, compound formula = N2O5.
Answer 3.
a.) Mass of Tin = W2-W1 = 24.67 - 22.36 = 2.31 grams.
b.) Mass of O = Mass of Tin Oxide - Mass of Tin = (W3-W1)-W2 = (24.98-22.36)-2.31 = 0.31 grams.
where W1 = mass of crucible and cover
W2 = mass of crucible, cover and Sn
W3 = mass of crucible, cover and tin oxide
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Pre-Laboratory Assignment 1. Why shouldn't you look directly at burning magnesium? 2. A compound composed of...
How do I calculate the emperical formula for the magnesium oxide compound? Empirical Formula of Magnesium...
How do I calculate the emperical formula for the
magnesium oxide compound?
Empirical Formula of Magnesium Oxide Compound Group Data: For these calculations, obtain the data shown on the previous page for two other groups. Make calculations here using your data and the data from the two other groups. Average Moles of Magnesium (mol) O. 0181 O.0025 Standard Deviation in Moles of Magnesium (mol) Average Moles of Oxygen (mol) rolo2 O. 00683 3:2 Standard Deviation in Moles of Oxygen (mol)...
help me solve please. im stumped EMPIRICAL FORMULA OF MAGNESIUM OXIDE COMPOUND INDIVIDUAL DATA Mass of...
help me solve please. im stumped
EMPIRICAL FORMULA OF MAGNESIUM OXIDE COMPOUND INDIVIDUAL DATA Mass of Empty Crucible (g) + lid 41.3549 47.4 Mass of the Magnesium (g) Mass of the Crucible with Contents After the Reaction (g) Mass of the Contents (Magnesium Oxide) Alone (g) 47.253941613 416959 4099 41 a 42.200 a 1.513 1o. 2719 10.1159 | 103 10.014 mol , 0168 ml 1.0169 10.017 mol 1.007 1.000644 Mass of the Oxygen in the Magnesium Oxide (g) Moles of...
As a result of this procedure, anything that was in the crucible at the end of...
As a result of this procedure, anything that was in the crucible at the end of the experiment, along with the magnesium oxide product, would cause an error in the figure that is recorded as "mass of oxygen". Would extra mass it the crucible cause the "mass of oxygen" to come out too high or too low? Explain. Here are some data from a similar experiment, to determine the empirical formula of an oxide of tin. Calculate the empirical formula...
NAME: DATE: SECTION/GROUP: INSTRUCTOR: DATA ANALYSIS OBSERVATIONS Anything you observed, condensation, steam, smoke, spilled compound, etc....
NAME: DATE: SECTION/GROUP: INSTRUCTOR: DATA ANALYSIS OBSERVATIONS Anything you observed, condensation, steam, smoke, spilled compound, etc. EMPIRICAL FORMULA OF MAGNESIUM OXIDE COMPOUND INDIVIDUAL DATA Mass of Empty Crucible (8) 42.9356 43.6656-42.1356 -0.73, Mass of the Magnesium (g) 3 Mass of the Crucible with Contents After the Reaction (g) | 44. 167g Mass of the Contents (Magnesium Oxide) Alone (8) Mass of the Oxygen in the Magnesium Oxide (g) Moles of Magnesium (mol) D 44.167 - 42.9351. = 1.259 ED-B 0.5g...
66 Laboratory Manual for General, Organic, and Biological Chemistry Questions and Problems 01 Using the rules...
66 Laboratory Manual for General, Organic, and Biological Chemistry Questions and Problems 01 Using the rules for writing the formulas of ionic compounds, write the ions and the correct formula for magnesium oxide. Ma 2 + + 0 2 = MgO Q2 Write a balanced equation for the reaction of the magnesium and the oxygen (02), including their physical states. Q3 Calculate the simplest formula for each of the following compounds: a. 0.200 mole of Al and 0.600 mole of...
Pestlab questions 1. Knowing what you do about magnesium and oxygen, what type of compound (lonie...
Pestlab questions 1. Knowing what you do about magnesium and oxygen, what type of compound (lonie or covalent) should form between these two elements? If you expect an ionic compound, comment on what ions will be bonding together, and in what ratio you expect based on their charges. Also, if that wasn't the ratio you obtained in your experiment, comment on possible sources of error 2. A student starts with a 3.96 sample of manganese (Mn, molar mass is 54.94...
1. A student who was in a hurry to complete this experiment did not follow the...
1. A student who was in a hurry to complete this experiment did not follow the exact directions for some of the procedural steps. Briefly explain what effect, if any, the following changes would have on the whole number ratio of Mg and O in the compound the student produced. (1) When arriving at the laboratory station, the student found a dirty crucible and cover. In the interest of time, the student skipped steps 2-8, weighed the cruible and cover,...
empirical formula of a compound Another Group's Data Your Group's Data ±o.oo! 1. Weight of dry crucible and cover 33 6029 2. Weight of dry crucible, cover, and metal 02 3. Weight of metal...
empirical formula of a compound
Another Group's Data Your Group's Data ±o.oo! 1. Weight of dry crucible and cover 33 6029 2. Weight of dry crucible, cover, and metal 02 3. Weight of metal 4. Weight of dry crucible, cover and metal oxide 5. Weight of metal oxide necal oxide 0-8 6. Weight of oxygen in metal oxide 上7120 aoung 7. Metal to oxygen mass ratio 8. Moles of metal 0001 Mole o166 mol 9. Moles of oxygen 0. Metal...
determinations - (1) mass of covered crucible and Mg, g (2) mass of crucible and cover,...
determinations - (1) mass of covered crucible and Mg, g (2) mass of crucible and cover, g P.8 g 17.355 0.45g 18.095 0.749 (3) mass of Mg, g - - - (4) mass of covered crucible and magnesium oxide, g (5) mass of magnesium oxide, (6) mass of O that combined with Mg, g (7) number of moles of Mg (8) number of moles of O (9) ratio of number of moles of Mg to the smaller of the two...
Experiment 3 Prelaboratory Assignment Empirical Formulas Date Lobo Sec. Name Desk No. 1. Elemental mercury was...
Experiment 3 Prelaboratory Assignment Empirical Formulas Date Lobo Sec. Name Desk No. 1. Elemental mercury was first discovered when a mercury oxide was decomposed with heat, forming mercury metal and oxygen gas. When a 0.204-g sample of the mercury oxide heated. 0.189 g of mercury metal remains. Note: not attempt this experiment in the laboratory because of the release of toxic mercury vapor. a. What is the mole ratio of mercury to oxygen in the sample? b. What is the...
How do I calculate the emperical formula for the
magnesium oxide compound?
Empirical Formula of Magnesium Oxide Compound Group Data: For these calculations, obtain the data shown on the previous page for two other groups. Make calculations here using your data and the data from the two other groups. Average Moles of Magnesium (mol) O. 0181 O.0025 Standard Deviation in Moles of Magnesium (mol) Average Moles of Oxygen (mol) rolo2 O. 00683 3:2 Standard Deviation in Moles of Oxygen (mol)...
help me solve please. im stumped
EMPIRICAL FORMULA OF MAGNESIUM OXIDE COMPOUND INDIVIDUAL DATA Mass of Empty Crucible (g) + lid 41.3549 47.4 Mass of the Magnesium (g) Mass of the Crucible with Contents After the Reaction (g) Mass of the Contents (Magnesium Oxide) Alone (g) 47.253941613 416959 4099 41 a 42.200 a 1.513 1o. 2719 10.1159 | 103 10.014 mol , 0168 ml 1.0169 10.017 mol 1.007 1.000644 Mass of the Oxygen in the Magnesium Oxide (g) Moles of...
As a result of this procedure, anything that was in the crucible at the end of the experiment, along with the magnesium oxide product, would cause an error in the figure that is recorded as "mass of oxygen". Would extra mass it the crucible cause the "mass of oxygen" to come out too high or too low? Explain. Here are some data from a similar experiment, to determine the empirical formula of an oxide of tin. Calculate the empirical formula...
NAME: DATE: SECTION/GROUP: INSTRUCTOR: DATA ANALYSIS OBSERVATIONS Anything you observed, condensation, steam, smoke, spilled compound, etc. EMPIRICAL FORMULA OF MAGNESIUM OXIDE COMPOUND INDIVIDUAL DATA Mass of Empty Crucible (8) 42.9356 43.6656-42.1356 -0.73, Mass of the Magnesium (g) 3 Mass of the Crucible with Contents After the Reaction (g) | 44. 167g Mass of the Contents (Magnesium Oxide) Alone (8) Mass of the Oxygen in the Magnesium Oxide (g) Moles of Magnesium (mol) D 44.167 - 42.9351. = 1.259 ED-B 0.5g...
66 Laboratory Manual for General, Organic, and Biological Chemistry Questions and Problems 01 Using the rules for writing the formulas of ionic compounds, write the ions and the correct formula for magnesium oxide. Ma 2 + + 0 2 = MgO Q2 Write a balanced equation for the reaction of the magnesium and the oxygen (02), including their physical states. Q3 Calculate the simplest formula for each of the following compounds: a. 0.200 mole of Al and 0.600 mole of...
Pestlab questions 1. Knowing what you do about magnesium and oxygen, what type of compound (lonie or covalent) should form between these two elements? If you expect an ionic compound, comment on what ions will be bonding together, and in what ratio you expect based on their charges. Also, if that wasn't the ratio you obtained in your experiment, comment on possible sources of error 2. A student starts with a 3.96 sample of manganese (Mn, molar mass is 54.94...
empirical formula of a compound
Another Group's Data Your Group's Data ±o.oo! 1. Weight of dry crucible and cover 33 6029 2. Weight of dry crucible, cover, and metal 02 3. Weight of metal 4. Weight of dry crucible, cover and metal oxide 5. Weight of metal oxide necal oxide 0-8 6. Weight of oxygen in metal oxide 上7120 aoung 7. Metal to oxygen mass ratio 8. Moles of metal 0001 Mole o166 mol 9. Moles of oxygen 0. Metal...
determinations - (1) mass of covered crucible and Mg, g (2) mass of crucible and cover, g P.8 g 17.355 0.45g 18.095 0.749 (3) mass of Mg, g - - - (4) mass of covered crucible and magnesium oxide, g (5) mass of magnesium oxide, (6) mass of O that combined with Mg, g (7) number of moles of Mg (8) number of moles of O (9) ratio of number of moles of Mg to the smaller of the two...
Experiment 3 Prelaboratory Assignment Empirical Formulas Date Lobo Sec. Name Desk No. 1. Elemental mercury was first discovered when a mercury oxide was decomposed with heat, forming mercury metal and oxygen gas. When a 0.204-g sample of the mercury oxide heated. 0.189 g of mercury metal remains. Note: not attempt this experiment in the laboratory because of the release of toxic mercury vapor. a. What is the mole ratio of mercury to oxygen in the sample? b. What is the...
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