A sample of H2 gas is collected over water by reacting zinc metal with a solution of hydrochloric acid (HCl). In addition to the hydrogen gas, a solution of zinc chloride is also formed. 1. Write the balanced chemical equation for the reaction. Include all states of matter.

2. Write the net ionic equation for this reaction. Include all states of matter.

3. Based on intermolecular forces, why is the H2 gas able to be collected over water rather than being dissolved in the water?

4. If a 0.25 g sample of Zn reacts with excess HCl…
How many moles of HCl will react?

5. How many moles of H2(g) should be produced?

6. The experiment takes place under the following conditions: 300 K, Patm = 777 mmHg, PH2O at 300 K = 26.7 mmHg. How many liters of H2 would be generated under these conditions from the reaction of 0.25 g Zn with excess HCl?

7. How would the amount of H2 collected change if the piece of zinc that reacted had a mass of 0.35 g? Explain.