Lab Report

1. How does the mass of AgNO3 formed at the start of this experiment compare with the mass used in the last experiment? How do you account for any difference?

Last experiment, we formed about a gram of AgNO3. During this experiment, the grams went up to 11.19g. There may be a difference because it is possible that we measured the grams wrong during the last experiment. Maybe the one gram amount should be something higher and much closer to 11.19g.

2. Silver chloride and sodium nitrate were the products formed when the reactants silver nitrate and sodium chloride were combined. From the value of your ratio in calculation #2, how does the mass of the products compare to the mass of the reactants?

There is a one to one ratio between the mass of the products and the mass of the reactants.

3. Note that the masses of Ag, AgNO3, and AgCl in this experiment are very different. However, what do the values of the ratios in calculation #3 reveal about the number of silver atoms involved in this series of chemical changes?

It reveals that there were a lot of silver atoms involved with this experiment. Silver reacts with other substances to get different masses. Silver seems to react very well with many different types of substances, such as nitrate and chloride.

4. If everything went perfectly, you would expect to recover 100% of the silver you started with in the last experiment. How do you explain your answer to calculation number four? Don't be vague!! If your answer is too low, try to explain at what points in the experiment that you might have lost silver. If your % is too high, explain how this could have happened.

If the answer was too low, we may have lost silver when we were transferring it into the beakers. We may have not measured the correct amount of silver to put into the beaker. If the answer was too high, again, we might have measured incorrectly. There could have also been spilling that could have caused the percentage to be too low.