Mole Conversions
Jerome was asked to perform the following chemical reaction. He placed 5.0g of zinc metal into a bottle and covered the mouth of the bottle with a 2-hole stopper. Jerome then assembled the laboratory setup. He poured 150 mL of 2.0 M HCL through the funnel onto the zinc. As the reaction proceeded, bubbles began to appear in the inverted bottle, displacing some of the water inside of the bottle.
Using your knowledge of molar quantities. Answer the following questions.
1.
a) Write the balanced equation for the reaction between the zinc and the acid.
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b) Indentify the type of reaction that has occured.
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2. a) Calculate the number of moles of zinc that Jerome placed in the bottle at the beginning of the experiment.
b) If all of the zinc reacts, the number of moles of zinc consumed will be the same as the number of moles of H2 (gas) produced. How many molecules of hydrogen gas will be produced in this reaction?
3. Calculate the volume of the hydrogen gas produced in this reaction at STP.
4. Calculate the mass of the hydroden that will be collected in the inverted bottle.
5. Predict the mass of the hydrogen that would have been produced if Jerome had started with twice the original mass of zinc. Assume that all of the zinc would react.