chemistry 40

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1.      Record the following: 

 

a. mol of Ag+                 107.87g

b. mol of NO3               62.01g

c. Total mol of AgNO3 170g

 

2.      Calculate the number of mol AgNO3 in 1.00 g AgNO3. Show your work.

 

3. Do you think using a big ‘carboy’ of water to pour 100. mL of solution is realistic?

 

a. Describe a more realistic way to obtain about 100 mL of water. 

 

 

 

 

b. Describe a more precise way to measure 100.0 mL water using the equipment available in the virtual lab.

 

 

 

 

Written Assignment 3:

1. Calculate the theoretical or expected yield from the reaction of 1.00 g NaCl and 1.00 g AgNO3. (Good thing to do while you wait for your reaction to finish.)

 

2. What is the Limiting Reagent?

 

 

3. When the reaction appears to stop, switch to the solid window and record the mass of AgCl formed.

 

 

4. What is the percent yield?

 

Written Assignment 4:

1. Record the following: 

a.      Mass of Na+                                       _________

b.      Mass of Cl                                          _________

c.       Total mass of NaCl                   _________

 

2. Use stoichiometry to calculate the grams of AgNO3 needed to react completely with the sodium chloride. (Show your work and use units too!)

 

 

3. Use stoichiometry (with units) to calculate the theoretical yield of AgCl formed in this reaction. (You only need to do the problem with one of the reactants since this is no limiting reagent in this reaction.)

 

 

4. Identify the actual yield of AgCl (in grams) from the species viewer.

5. What is the Percent Yield of the reaction?

 

 

Written Assignment 5:

1. Calculate the theoretical yield (expected yield) when 0.800 g solid NaCl is added to the 3.00 g AgNO3 solution Show your calculations.

 

 

2. What is the limiting reagent in this problem?

 

 

 

3. What is the percent yield?

 

 

 

 

 

4. Do any of your experimental results worry you based on your analysis of the percent yields?  Why? (Recall that a percent yield is not the same as a percent error.

 

 

5. Discuss how and why the results in your experiments is are likely to differ in a physical lab.

 

 

 

 

Problems:

Given the reaction:

3 CaCl2 (aq) + 2 Na3PO4 (aq)     Ca3(PO4)2 (s) + 6 NaCl (aq)

a. If solutions containing 400.0 g CaCl2 and 400.0 g Na3PO4  are mixed, how much (g) Ca3(PO4)2can be formed?

b. What is the Limiting Reagent?

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