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3. What is the mole ratio of salt to water for the following compounds? Hydrate Salt Water CaCl2 - 2 H20 FeSO4 · 7...
chemistry
A student was in a hurry and decided to take a shortcut in the Procedure. After washing and drying the crucible with towels, the student did not do steps 2, 3, and 4 in the Procedure, but immediately went to step 5 and continued from there. What is the error that will be introduc into the experiment? 2. If your sample contained a volatile impurity, what value would be in error, the mass of the anhydrous salt or the mass...
4. A student worked with a sample of ZnSO4.7H2O. a. How many atoms of each kind...
4. A student worked with a sample of ZnSO4.7H2O. a. How many atoms of each kind are present? b. What is the stoichiometric ratio of salt to water? c. Calculate the percent of water in the hydrate. Show your work.
Post-Lab Questions 1. A student was in a hurry and decided to take a shortcut in...
Post-Lab Questions 1. A student was in a hurry and decided to take a shortcut in the Procedure. After washing and drying the crucible with towels, the student did not do steps 2, 3, and 4 in the Procedure, but immediately went to step 5 and continued from there. What is the error that will be introduc into the experiment? 2. If your sample contained a volatile impurity, what value would be in error, the mass of the anhydrous salt...
determining the formula of a hydrate of calcium chloride (CaCl2·X H2O). Mass (g) Crucible and Lid...
determining the formula of a hydrate of calcium chloride (CaCl2·X H2O). Mass (g) Crucible and Lid 28.4735 Crucible and Lid + hydrate salt 33.1938 Crucible and Lid + anhydrous residue 32.0339 What is the mass of the hydrate? mass = ___ g What is the mass of the anhydrous residue? mass = ___ g What is the mass of water lost upon heating the sample? mass = ___ g How many mol of H2O were lost upon heating? (H2O: 18.016...
1. what is the mole ratio for trial 1 and 2? 2. whats the average mole...
1. what is the mole ratio for trial 1 and 2?
2. whats the average mole ratio for trial 1 and
2?
3. whats the average deviation for trial 1 and 2?
* please include the steps if you dont mind*
ng down the equation ahd an example calculation, The example calculation only needs to be done for one trial. The results of the remaining trials can be written down in a table in your notebook. (Part 1)) Determine the...
A student heated a sample of a hydrated salt and obtained the following data: Grams of...
A student heated a sample of a hydrated salt and obtained the following data: Grams of hydrated salt used: 1.0000 gram Grams of anhydrous salt (147 g/mole) recovered: 0.8033 grams Grams of water vapour (18 g/mole) lost: 0.1967 grams Determine the percentage by mass of water in this hydrate. (1) How many water molecules, "X", are bonded to this hydrated salt, salt. X H20? (2)
Experiment 3: Determination of Percent Water in a Hydrate Data Sheet Run #1 Run #2 _37.032...
Experiment 3: Determination of Percent Water in a Hydrate Data Sheet Run #1 Run #2 _37.032 g Mass of crucible and cover 38.067 g Mass of crucible, cover and hydrate Mass of hydrate taken for 2-1- analysis 38.Ona _37.713 g Mass of crucible, cover and residue (after heating) _8 - Mass of H20 lost 6. _(FW=18.015 g/mol) mol Moles of H20 lost 13 3521 % % Percent of H20 lost .8 Mass of residue (anhydrous salt) mol Moles of anhydrous...
A student is given a sample of a manganese(II) chloride hydrate. She weighs the sample in...
A student is given a sample of a manganese(II) chloride hydrate. She weighs the sample in a dry, covered crucible and obtains a mass of 24.747 g for the crucible, cover, and sample. Earlier she had found that the crucible and cover weighed 23.599 g. She then heats the crucible to drive off the water of hydration, keeping the crucible at red heat for about 10 minutes with the cover slightly ajar. She then lets the crucible cool, and finds...
CHM 010 On-Line Lab, Formula of a Hydrate PURPOSE: To determine the formula of Cuso..x H20....
CHM 010 On-Line Lab, Formula of a Hydrate PURPOSE: To determine the formula of Cuso..x H20. In other words, to determine the value of "X". PROCEDURE: When copper(II) sulfate x hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as anhydrous copper(II) sulfate. The "x" represents a whole number of water molecules attached to...
The example given the following problem: I used 1.50 grams of the CaCl2•2H2O. I just want...
The example given the following problem:
I used 1.50 grams of the
CaCl2•2H2O.
I just want to make sure I did my calculations right?
Could someone please review my answers and provide appropriate
feedback my their answers to mine differ?
If they do, can you show your work.
A step-by-step example of this process, using the balanced equation from Figure 1, is shown below: CuSO4(aq)2NaOH(aq) -> Cu(OH)2(s) Na2SO4(aq) Assuming there are only 5.70 grams of CuSO4 available, how many grams...
4. A student worked with a sample of ZnSO4.7H2O. a. How many atoms of each kind are present? b. What is the stoichiometric ratio of salt to water? c. Calculate the percent of water in the hydrate. Show your work.
Post-Lab Questions 1. A student was in a hurry and decided to take a shortcut in the Procedure. After washing and drying the crucible with towels, the student did not do steps 2, 3, and 4 in the Procedure, but immediately went to step 5 and continued from there. What is the error that will be introduc into the experiment? 2. If your sample contained a volatile impurity, what value would be in error, the mass of the anhydrous salt...
1. what is the mole ratio for trial 1 and 2?
2. whats the average mole ratio for trial 1 and
2?
3. whats the average deviation for trial 1 and 2?
* please include the steps if you dont mind*
ng down the equation ahd an example calculation, The example calculation only needs to be done for one trial. The results of the remaining trials can be written down in a table in your notebook. (Part 1)) Determine the...
A student heated a sample of a hydrated salt and obtained the following data: Grams of hydrated salt used: 1.0000 gram Grams of anhydrous salt (147 g/mole) recovered: 0.8033 grams Grams of water vapour (18 g/mole) lost: 0.1967 grams Determine the percentage by mass of water in this hydrate. (1) How many water molecules, "X", are bonded to this hydrated salt, salt. X H20? (2)
Experiment 3: Determination of Percent Water in a Hydrate Data Sheet Run #1 Run #2 _37.032 g Mass of crucible and cover 38.067 g Mass of crucible, cover and hydrate Mass of hydrate taken for 2-1- analysis 38.Ona _37.713 g Mass of crucible, cover and residue (after heating) _8 - Mass of H20 lost 6. _(FW=18.015 g/mol) mol Moles of H20 lost 13 3521 % % Percent of H20 lost .8 Mass of residue (anhydrous salt) mol Moles of anhydrous...
A student is given a sample of a manganese(II) chloride hydrate. She weighs the sample in a dry, covered crucible and obtains a mass of 24.747 g for the crucible, cover, and sample. Earlier she had found that the crucible and cover weighed 23.599 g. She then heats the crucible to drive off the water of hydration, keeping the crucible at red heat for about 10 minutes with the cover slightly ajar. She then lets the crucible cool, and finds...
CHM 010 On-Line Lab, Formula of a Hydrate PURPOSE: To determine the formula of Cuso..x H20. In other words, to determine the value of "X". PROCEDURE: When copper(II) sulfate x hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as anhydrous copper(II) sulfate. The "x" represents a whole number of water molecules attached to...
The example given the following problem:
I used 1.50 grams of the
CaCl2•2H2O.
I just want to make sure I did my calculations right?
Could someone please review my answers and provide appropriate
feedback my their answers to mine differ?
If they do, can you show your work.
A step-by-step example of this process, using the balanced equation from Figure 1, is shown below: CuSO4(aq)2NaOH(aq) -> Cu(OH)2(s) Na2SO4(aq) Assuming there are only 5.70 grams of CuSO4 available, how many grams...
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