Experiment 1 Mass Of Zinc 0 25g Vol Of 6m Hci 10ml Vol Of Hydrogen Gas Produced 92 3 2851425

Experiment 1 Mass of Zinc: 0.25g Vol of 6M HCI 10mL Vol of hydrogen gas produced: 92.3mL Temperature 21.5C Pressure: 1.00atm Experiment 2 Mass of Zinc: 0.5g Vol of 6M HCI 10mL Vol of hydrogen gas 184.5ml Terperature 27.4C Pressure: 1.68atm 1. How many moles of zinc reacted with the 6M HCl in the second part of the experiment? To find the moles of zinc you need to convert from the grams of zinc to the moles of zinc using the following calculation: moles of Zn = g of zinc * (1 mol Zn/molecular weight of Zn) 2. How many moles of H2 were produced in the first part of the experiment? Notice from the reaction given in the procedures that for every mole of zinc, there is one mole of H2 produced. 3. You have recorded the volume of hydrogen gas produced in the reaction and you have calculated the number of moles used in the second part of the experiment. Based on this information, what is the molar volume of hydrogen gas at room temperature? To calculate this, use the formula: Molar volume (L/mol) = (measured volume)/(number of moles). Remember to convert your measured volume from mL into L (1L = 1000mL). 4. The molar volume of an ideal gas at 21oC is listed in the Background section of the lab manual as 24.137L/mol. Compare your measured value to the listed value by calculating the experimental error from the second part of the experiment according to the formula: % error = | experimental molar volume – listed molar volume | / (listed molar volume) * 100% 5. Which was the limiting reactant: the zinc or the hydrochloric acid? Remember that the limiting reactant is completely consumed in a reaction and no new product is formed unless more of the limiting reactant is added. 6. In the second part of the experiment you used twice the amount of zinc as in the first part of the experiment. What affect did this have on the amount of hydrogen gas that was evolved in part 2 of the experiment? 7. If you were to use 25 moles of zinc in this experiment, how many moles of hydrogen gas would be produced? 8. In the production of ammonia via the Haber process, nitrogen gas is combined with hydrogen gas according to the following reaction: N2(g) + 3H2(g) -> 2NH3(g) If 50 moles of nitrogen gas were used in the reaction (and there was excess hydrogen gas), how many moles of ammonia could be generated? 9. You perform an experiment at 21oC and 1atm of pressure and generate helium gas in the laboratory. What do you expect the molar volume of the helium to be?

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