-
Heating 1.29 g of gallium gives a gallium-oxygen compound with a mass of 1.73 g.
-How many grams of oxygen are in the 1.73 grams of gallium-oxygen compound.
-
Lab #19; Empirical Formula of Magnesium Hydroxide Pre-Lab Questions Name: Heating 1.29 g of gallium gives a gallium-oxygen compound with a mass of 1.739 Calculate the empirical formula of the compound. Step 1: Figure out how many grams of oxygen are in the 1.73 grams of gallium-oxygen compound. Step 2: Convert the 1.29 g of gallium to moles: Step 3: Convert the grams of oxygen you calculated in step 1 to moles: Step 4: Figure out the formula. Formula Name
-
Please answer all parts
7. Gallium sulfide is a compound that is used as a semiconductor in electronics. It is synthesized from elemental gallium and sulfur, according to the following balanced chemical equation: (14 Points) 2 Ga (s) + 3 S (s) → Ga2S3 (s) a. What is the theoretical yield (in grams) of GazSz if 4.53 g of gallium reacts with 3.25 g of sulfur? [Given molar masses: Ga 69.72 g/mol; S 32.07 g/mol; Ga2S3 253.65 g/molj c. What...
-
A compound contains only carbon, hydrogen, and oxygen.
Combustion of 18.92 g of the compound yields 27.73 g of CO2 and
11.35 g of H2O. The molar mass of the compound is 90.078 g/mol.
*Each part of this problem should be submitted separately to avoid
losing your work*
1. Calculate the grams of carbon (C) in 18.92 g of the compound:
grams
2. Calculate the grams of hydrogen (H) in 18.92 g of the
compound. grams
3. Calculate the grams...
-
7. A compound contains 30.4 g of nitrogen and 69.6 g of oxygen by mass. What is the chemical formula of this compound? 8. How many molecules of H,O (M.w. 18 g/mol) are there in 355 grams of H,O? How many hydrogen atoms are in 355 grams of HO?
-
1. When 2.50 g of copper metal reacts with molecular oxygen, the copper oxide product of the reaction has a mass of 2.81 g. What is the empirical formula of the copper oxide product 2. When 10.8 g of silver was reacted with sulfur. 12.4 grams of product was produced there was only one product). What is the empirical formula of the product? 3. Lysine is a compound composed of carbon, hydrogen, nitrogen and oxygen. When 1.50 g of lysine is burned,...
-
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...
-
please help me with the second column.
Lab Data Sheet 1. Mass of lid (9) Trial 1 6.66904 39.65269 40.29104 Trial 2 16.4783 38.0139 32.54279 2. Mass of crucible and lid (9) 3. Mass of crucible, lid, and magnesium(g) 4. Mass of crucible, lid and compound 1st mass measurement (g) 40.77679 90.47004 38.8188 38.81319 2nd mass measurement (g) 3rd mass measurement (9) CALCULATIONS Trial 2 5383 Trial .89559 •0368 1.1644 1. Mass of Magnesium (9) 2. Moles of Magnesium (mol)...
-
Calculate the heat evolved when 0.500 g of Cl, (g) reacts with an excess of HBr (g) to form HCI (g) and Br, (0, given the following standard enthalpies of formation (kJ/mol): HCI (B), - 92.30; HBr (g), -36.20. Ryan Experiment 4 Advance Study Assignment: Determination of a Chemical Formula 1. To find the mass of a mole of an element, one looks up the atomic mass of the element in a table of atomic masses (see Appendix III or...
-
Question 4 (1 point) A compound with a molecular mass of 283.88 g/mol is found to contain 43.64 %P and 56.36% O. What is the molecular formula of this compound? OPO4 OP203 P205 OP4010 OPAOG Question 5 (1 point) If (4.544x10^1) g of oxygen react with (4.81x10^1) g of carbon monoxide to form carbon dioxide. What mass of carbon dioxide forms? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: Answer