Additional Questions 1. What was the limiting reactant? Give specific visible ev

Question

Additional Questions 1. What was the limiting reactant? Give specific visible evidence to support your answer. Would the experimental results for moles of copper and for moles of chlorine increase, decrease, or remain the same in the following situations? Clearly explain your reasoning. (Two separate answers are needed for each: moles Cu and moles Cl.) You stopped the reaction early, while the solution was still pale blue. You used two pieces of zinc (rather than one) and had much more zinc left when the reaction finished. If you mistakenly performed the procedure using 0.50 g of copper chloride (rather than 1.00 g), how would this change your answer for the empirical formula? Clearly explain your reasoning. Calculate the number of potassium atoms present in: 0.2500 g of potassium metal. 0.2500 g of KNO3.

Explanation / Answer

4.

a. Number of potasssiun atoms present in 0.2500 g of potassium metal

moles of poatassium = g/molar mass

= 0.2500g/39.0983

= 6.39 x 10^-3 mols

So atoms of potassium present would be = 6.39 x 10^-3 x 6.022 x 10^-23

= 3.85 x 10^21 atoms

b. 0.2500 g of KNO3

moles of KNO3 = 0.2500g/101.1032

= 2.47 x 10^-3 mols

Now, 1 mole of KNO3 has 1 mole of potassium in it.

So moles of potassium = 2.47 x 10^-3 mols

Atoms of potassium = 2.47 x 10^-3 x 6.022 x 10^23

= 1.49 x 10^21 atoms

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