Using the data recorded in table 1. Calculate and fill out table 2. Table 1: Gas Laws and Molar Volume of Ideal Gas DataInitial TemperatureItem Measuredmass of zinc used (g)volume of 6.0 M HCI used(mL)ExperimentTrial #10.100 g45.00 mLpressure in the flask beforeadding the gas syringe (atm)volume of gas produced (mL) 36.83 mLInitial Pressure1.139 atmExperiment ExperimentTrial #2Trial #30.200 g45.00 mL1.280 atm73.63 ml1.000 g45.00 mL1.000 atm0.00 mLExperimentTrial #4(your choiceof values)0.150 g45.00 mL1.210 atm55.22 mL Table 2: Gas Laws and Molar Volume of Ideal Gas Calculated ValuesMolar Mass of Gas ) producedMolar Mass of ZincDetermined Valuemoles of zinc reactedmoles of hydrogen producedmolar volume of the gas produced atroom temperaturetheoretical yield of molar gas producedproducedPercent ErrorExperiment Experiment Experiment ExperimentTrial#1 Trial#2 Trial#3 Trial#4

The number of moles of a substance is the ratio of the mass of the substance to the molar mass of the substance. The number of moles when concentration and the volume are given. The reaction between Zn and HCl is From the balanced equation, it is clear that one mole of Zn requires 2 mol of HCl and produces one equivalent of hydrogen gas. Molar mass of Zn is 65.38 g/mol. Molar mass of H2 is 2.016 g/mol. Determination of the number of moles of Zn reacted. The number of moles of Zn can be calculated as follows. The mass of Zn is 0.100 g and the molar mass of Zn is 65.38 g/mol. To find the number of moles of Zn reacted, we also have to find the number of moles of HCl present. The number of moles of HCl can be calculated as follows. The concentration of HCl is 6.0 M and the volume of HCl is 45.00 mL. From the balanced equation, 0.27 mol HCl requires of Zn. Since that much Zn is not present, Zn is the limiting reagent. Hence, Zn undergoes complete conversion. So, of Zn reacts. From the balanced equation, one mole of Zn produces one mole of H2. So, number of moles of H2 is the same as the number of moles of Zn. So, the number of moles of H2 is . The molar volume is the ratio of volume to the number of moles. So, the volume of gas produced is 36.83 mL. The number of moles of H2 is . So, the molar volume is The molar volume is 24.55 LThe molar volume at room temperature (298 K)can be calculated as follows. The pressure is 1.139 atm. The number of moles is 1. Universal gas constant, R is 0.0821 atm.L/(K.mol). Where P is pressure, V is volume, n is the number of moles, R is universal gas constant, and T is temperature. 'The theoretical volume is 21.48 L. The percent error is calculated as follows. The percent error is 14.3%. Determination of the number of moles of Zn reacted. The number of moles of Zn can be calculated as follows. The mass of Zn is 0.200 g and the molar mass of Zn is 65.38 g/mol. To find the number of moles of Zn reacted, we also have to find the number of moles of HCl present. The number of moles of HCl can be calculated as follows. The concentration of HCl is 6.0 M and the volume of HCl is 45.00 mL. From the balanced equation, 0.27 mol HCl requires of Zn. Since that much Zn is not present, Zn is the limiting reagent. Hence, Zn undergoes complete conversion. So, of Zn reacts. From the balanced equation, one mole of Zn produces one mole of H2. So, number of moles of H2 is the same as the number of moles of Zn. So, the number of moles of H2 is . The molar volume is the ratio of volume to the number of moles. So, the volume of gas produced is 73.63 mL. The number of moles of H2 is . So, the molar volume is The molar volume is 24.06 LThe molar volume at room temperature (298 K)can be calculated as follows. The pressure is 1.280 atm. The number of moles is 1. Universal gas constant, R is 0.0821 atm.L/(K.mol). The theoretical volume is 19.12 L. The percent error is calculated as follows. The percent error is 25.84%. Determination of the number of moles of Zn reacted. The number of moles of Zn can be calculated as follows. The mass of Zn is 0.200 g and the molar mass of Zn is 65.38 g/mol. To find the number of moles of Zn reacted, we also have to find the number of moles of HCl present. The number of moles of HCl can be calculated as follows. The concentration of HCl is 6.0 M and the volume of HCl is 45.00 mL. From the balanced equation, 0.27 mol HCl requires of Zn. Since that much Zn is not present, Zn is the limiting reagent. Hence, Zn undergoes complete conversion. So, 0.0153 mol of Zn reacts. From the balanced equation, one mole of Zn produces one mole of H2. So, number of moles of H2 is the same as the number of moles of Zn. So, the number of moles of H2 is 0.0153 mol. The molar volume is the ratio of volume to the number of moles. So, the volume of gas produced is 0.00 mL. The number of moles of H2 is 0.0153 mol. So, the molar volume is The molar volume is 0 L. Some error is made while determining this data by the student. The molar volume at room temperature (298 K)can be calculated as follows. The pressure is 1.280 atm. The number of moles is 1. Universal gas constant, R is 0.0821 atm.L/(K.mol). The theoretical volume is 24.47 L. The percent error is calculated as follows. The percent error is 100%. Determination of the number of moles of Zn reacted. The number of moles of Zn can be calculated as follows. The mass of Zn is 0.150 g and the molar mass of Zn is 65.38 g/mol. To find the number of moles of Zn reacted, we also have to find the number of moles of HCl present. The number of moles of HCl can be calculated as follows. The concentration of HCl is 6.0 M and the volume of HCl is 45.00 mL. From the balanced equation, 0.27 mol HCl requires of Zn. Since that much Zn is not present, Zn is the limiting reagent. Hence, Zn undergoes complete conversion. So, of Zn reacts. From the balanced equation, one mole of Zn produces one mole of H2. So, number of moles of H2 is the same as the number of moles of Zn. So, the number of moles of H2 is . The molar volume is the ratio of volume to the number of moles. So, the volume of gas produced is 0.00 mL. The number of moles of H2 is 0.0153 mol. So, the molar volume is The molar volume at room temperature (298 K)can be calculated as follows. The pressure is 1.210 atm. The number of moles is 1. Universal gas constant, R is 0.0821 atm.L/(K.mol). The theoretical volume is 20.22 L. The percent error is calculated as follows. The percent error is 19.24%. The table can be summarized as Molar mass of Zn is 65.38 g/mol. Molar mass of gas (H2) is 2.016 g/mol. Determined valueexperiment trial 1experimenttrial 2experimenttrial 3experiment trial 4Moles of zinc reacted0.0153 molmoles of hydrogen produced0.0153 molmolar volume of the gas produced at room temperature24.55 L24.06 L0 L24.11 Ltheoretical yield of molar gas produced21.48 L19.12 L24.47 L20.22 Lpercent error14.3%25.84%100%19.24%