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STP Calculations: 1) From your data, calculate the number of moles of hydrogen gas produced from mass of magnesium. Mg(s) + 2HCl(aq) = MgCl2(aq) + H2(g) Run 1 0.044g Mg I mot Mg x 1 mol H₂ Run 2 >>> Equation 1 =0.0018 mol H₂ I mot Mg=0.0015 mol H₂ 24 g Mg met Mg 0.035 g Mg 24 I mot Mg, I mol H₂ 24g Mg P-1.00a2) From your data, calculate the number of liters of hydrogen gas at Standard Pressure and Standard Temperature, or V2. The following formula is referred to as the Combined Gas T-0.00°C law, this is perhaps the most fundamental of all gas formulas, and one of the most useful. 273K Imol 22.4L Pmax -Pol Flask (L) P₁V₁ P₂V₂ T₁(K) T₂(k) 1.00 atm Overage The variable Pi is your pressure of hydrogen gas you produced in the reaction. P = Pre-Prim Phydrogen P1, this is the pressure of hydrogen gas you generated in the reaction. You subtract your maximum hydrogen pressure from atmospheric pressure, in kPa or atm Vi is the volume of the flask you carried the experiment out in, in liters Ti is the mean temperature of the hydrogen gas in this experiment, in Kelvin. P2 is the Standard Pressure, this is a constant, so never changes and is 101 kPa or 1 atm V2 is what you want to solve for, in liters T2 is the Standard Temperature, also, this never changes and is 273 K Fill in the values then solve for the Standard Volume of a gas (V2) in liters. SHOW YOUR CALC! P₁ = atm V₁ = 3 L T₁ = k P₂ = 1.00 atm V2= T2 = 273 k 70

STP Calculations: 1) From your data, calculate the number of moles of hydrogen gas produced from mass of magnesium. Mg(s) + 2HCl(aq) = MgCl2(aq) + H2(g) Run 1 0.044g Mg I mot Mg x 1 mol H₂ Run 2 >>> Equation 1 =0.0018 mol H₂ I mot Mg=0.0015 mol H₂ 24 g Mg met Mg 0.035 g Mg 24 I mot Mg, I mol H₂ 24g Mg P-1.00a2) From your data, calculate the number of liters of hydrogen gas at Standard Pressure and Standard Temperature, or V2. The following formula is referred to as the Combined Gas T-0.00°C law, this is perhaps the most fundamental of all gas formulas, and one of the most useful. 273K Imol 22.4L Pmax -Pol Flask (L) P₁V₁ P₂V₂ T₁(K) T₂(k) 1.00 atm Overage The variable Pi is your pressure of hydrogen gas you produced in the reaction. P = Pre-Prim Phydrogen P1, this is the pressure of hydrogen gas you generated in the reaction. You subtract your maximum hydrogen pressure from atmospheric pressure, in kPa or atm Vi is the volume of the flask you carried the experiment out in, in liters Ti is the mean temperature of the hydrogen gas in this experiment, in Kelvin. P2 is the Standard Pressure, this is a constant, so never changes and is 101 kPa or 1 atm V2 is what you want to solve for, in liters T2 is the Standard Temperature, also, this never changes and is 273 K Fill in the values then solve for the Standard Volume of a gas (V2) in liters. SHOW YOUR CALC! P₁ = atm V₁ = 3 L T₁ = k P₂ = 1.00 atm V2= T2 = 273 k 70

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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STP Calculations: 1) From your data, calculate the number of moles of hydrogen gas produced from mass of magnesium. Mg(s) + 2HCl(aq) = MgCl2(aq) + H2(g) Run 1 0.044g Mg I mot Mg x 1 mol H₂ Run 2 >>> Equation 1 =0.0018 mol H₂ I mot Mg=0.0015 mol H₂ 24 g Mg met Mg 0.035 g Mg 24 I mot Mg, I mol H₂ 24g Mg P-1.00a2) From your data, calculate the number of liters of hydrogen gas at Standard Pressure and Standard Temperature, or V2. The following formula is referred to as the Combined Gas T-0.00°C law, this is perhaps the most fundamental of all gas formulas, and one of the most useful. 273K Imol 22.4L Pmax -Pol Flask (L) P₁V₁ P₂V₂ T₁(K) T₂(k) 1.00 atm Overage The variable Pi is your pressure of hydrogen gas you produced in the reaction. P = Pre-Prim Phydrogen P1, this is the pressure of hydrogen gas you generated in the reaction. You subtract your maximum hydrogen pressure from atmospheric pressure, in kPa or atm Vi is the volume of the flask you carried the experiment out in, in liters Ti is the mean temperature of the hydrogen gas in this experiment, in Kelvin. P2 is the Standard Pressure, this is a constant, so never changes and is 101 kPa or 1 atm V2 is what you want to solve for, in liters T2 is the Standard Temperature, also, this never changes and is 273 K Fill in the values then solve for the Standard Volume of a gas (V2) in liters. SHOW YOUR CALC! P₁ = atm V₁ = 3 L T₁ = k P₂ = 1.00 atm V2= T2 = 273 k 70
Transcribed Image Text:STP Calculations: 1) From your data, calculate the number of moles of hydrogen gas produced from mass of magnesium. Mg(s) + 2HCl(aq) = MgCl2(aq) + H2(g) Run 1 0.044g Mg I mot Mg x 1 mol H₂ Run 2 >>> Equation 1 =0.0018 mol H₂ I mot Mg=0.0015 mol H₂ 24 g Mg met Mg 0.035 g Mg 24 I mot Mg, I mol H₂ 24g Mg P-1.00a2) From your data, calculate the number of liters of hydrogen gas at Standard Pressure and Standard Temperature, or V2. The following formula is referred to as the Combined Gas T-0.00°C law, this is perhaps the most fundamental of all gas formulas, and one of the most useful. 273K Imol 22.4L Pmax -Pol Flask (L) P₁V₁ P₂V₂ T₁(K) T₂(k) 1.00 atm Overage The variable Pi is your pressure of hydrogen gas you produced in the reaction. P = Pre-Prim Phydrogen P1, this is the pressure of hydrogen gas you generated in the reaction. You subtract your maximum hydrogen pressure from atmospheric pressure, in kPa or atm Vi is the volume of the flask you carried the experiment out in, in liters Ti is the mean temperature of the hydrogen gas in this experiment, in Kelvin. P2 is the Standard Pressure, this is a constant, so never changes and is 101 kPa or 1 atm V2 is what you want to solve for, in liters T2 is the Standard Temperature, also, this never changes and is 273 K Fill in the values then solve for the Standard Volume of a gas (V2) in liters. SHOW YOUR CALC! P₁ = atm V₁ = 3 L T₁ = k P₂ = 1.00 atm V2= T2 = 273 k 70
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