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After heating, the anhydrous salt can be left on the bench several minutes before weighing * True False A calcium chloride hydrate has a mass of 4.72 g. This sample is heated until no water remains. The CaCl2 anhydrous has a mass of 3.56 g. The formula of the hydrate is: (Molar mass CaCl2 = 111g/mol) %3D

After heating, the anhydrous salt can be left on the bench several minutes before weighing * True False A calcium chloride hydrate has a mass of 4.72 g. This sample is heated until no water remains. The CaCl2 anhydrous has a mass of 3.56 g. The formula of the hydrate is: (Molar mass CaCl2 = 111g/mol) %3D

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...
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18:46 ull A docs.google.com After heating, the anhydrous salt can be left on the bench several minutes before weighing True False A calcium chloride hydrate has a mass of 4.72 g. This sample is heated until no water remains. The CaCl2 anhydrous has a mass of 3.56 g. The formula of the hydrate is: (Molar mass CaCl2 = 111g/mol) CaC12.2H20 CaC12.H20 CaCl2.4H20 O Cac12.3H2O The formula of the hydrate is: (Molar mass of BaCl2=208.23g/mol), M(H2O) = 18g/mol To determine the value of x in the formula of the hydrate BaCl,xH;O, a student heated a sample of the hydrate in a crucible over a Bunsen burner to remove all the water and recorded the following data: Mass of the empty crucible 22.36 g Mass of the crucible + hydrate 32.23 g Mass of the crucible + anhydrous BaCl 30.20 g BaCl2.3H20 BaCl2.2H20 BaCl2.4H20 BaC12.H20
Transcribed Image Text:18:46 ull A docs.google.com After heating, the anhydrous salt can be left on the bench several minutes before weighing True False A calcium chloride hydrate has a mass of 4.72 g. This sample is heated until no water remains. The CaCl2 anhydrous has a mass of 3.56 g. The formula of the hydrate is: (Molar mass CaCl2 = 111g/mol) CaC12.2H20 CaC12.H20 CaCl2.4H20 O Cac12.3H2O The formula of the hydrate is: (Molar mass of BaCl2=208.23g/mol), M(H2O) = 18g/mol To determine the value of x in the formula of the hydrate BaCl,xH;O, a student heated a sample of the hydrate in a crucible over a Bunsen burner to remove all the water and recorded the following data: Mass of the empty crucible 22.36 g Mass of the crucible + hydrate 32.23 g Mass of the crucible + anhydrous BaCl 30.20 g BaCl2.3H20 BaCl2.2H20 BaCl2.4H20 BaC12.H20
18:46 ull A docs.google.com The rate of iodination of acetone for a concentration of iodine [12]= 0.03 M and a time = 730s is equal : * 4.11 x 10-5 M.s-1 4.11 x 10-6 M-1.s-1 4.11 x 10-5 M-1.s-1 4.11x10-6 M.s-1 If you do not understand a direction or part of a lab procedure: * Skip it and go on to the next part Try several methods until something works Ask the instructor before proceeding Figure it out as you do the experiment The correct answer for this operation: 1.05 + 5.1 + 8 is: * O 14.15 O 14 O 15 O 14.2
Transcribed Image Text:18:46 ull A docs.google.com The rate of iodination of acetone for a concentration of iodine [12]= 0.03 M and a time = 730s is equal : * 4.11 x 10-5 M.s-1 4.11 x 10-6 M-1.s-1 4.11 x 10-5 M-1.s-1 4.11x10-6 M.s-1 If you do not understand a direction or part of a lab procedure: * Skip it and go on to the next part Try several methods until something works Ask the instructor before proceeding Figure it out as you do the experiment The correct answer for this operation: 1.05 + 5.1 + 8 is: * O 14.15 O 14 O 15 O 14.2
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