1. conditions. a) reaction: H Calculate the molar volume of H, gas under experimental b) -0.421...

 

Transcribed Image Text:

1. conditions. a) reaction: H₂ Calculate the molar volume of H, gas under experimental b) -0.421 g Zn x _Lmol Zn Lmol H, 0.00644 mol 65.39 g Zn 1 mol Zn Second, the molar volume under experimental conditions is determined by taking the ratio of the volume of H, gas (in L) collected by the n mol H₂. The volume of H, gas is calculated from the total volume collected, taking into account the fact that a small percentage of the total volume is due to the presence of water vapor. By taking the ratio of the P over the P₁, we have the volume fraction of H, gas, which, when multiplied by the total volume, yields the volume of H, gas collected. PPT - Po=769 torr-16.5 torr=752.5 torr First, determine the n mol of H, gas generated by the The molar volume of H, gas under experimental conditions can now be calculated as follows: VH-752.5 torr x 0.156 L-0.153 L 769 torr 0.153 L 0.00644 mol H₂ 2. Calculate the molar volume of H, gas under STP 3. conditions. V₁ 23.8 L/mol Under experimental conditions: Pon = 752.5 torr (= P₁₂) Tor = 19.0°C +273 = 292 K Von Under STP conditions: VSTP Psir TSTP To calculate the molar volume under STP conditions, use the formula of the combined gas law shown below. The accepted value molar volume of an ideal gas is 22.4 L/mol. -0.153 L Calculate the universal gas constant, R. under experimental conditions. = 23.8 L/mol = 1 atm = 760 torr - 0°C -273 K T₁₂ - 292 K -0.00644 mol Use the following formula to calculate R: PHZ-752.5 torr x Latm- 0.990 atm 760 torr LAB ASSIGNMENT In this lab, the following reaction between Mg metal and excess aqueous HCI is being studied: Mg(s) + 2 HCl(aq) MgCl₂(aq) + H₂(g) To start the reaction, a mass of 0.0118 g of Mg is initially added to the reaction vessel. The H₂ gas produced is collected over water. The volume of gas collected is 11.86 mL, and a gas pressure of 776 torr is measured at 23 °C. The vapor pressure of water at 23 °C is 21 torr. Using the above information, answer the questions in the boxed areas beginning on page 4. Question 1: (5 pts) Calculate the molar volume of H₂ gas generated under experimental conditions. Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Question 2 Part A: (5 pts) Calculate the molar volume of H₂ gas generated under STP conditions Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Part B: (0.5 pt) Given that accepted value of molar volume under STP conditions is 22.4 L/mol, calculate the percent error. If the answer is negative, take the absolute value to express it as positive. Show calculation set-up and round off the answer to correct sig figs. Answers without proof of calculations will receive no credit. Question 3 Part A: (5 pts) Calculate the Universal Gas Constant, R, under experimental conditions Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Part B: (0.5 pt) Given that accepted value of the universal gas constant is 0.08206 Lxatm/molxK, calculate the percent error. If the answer is negative, take the absolute value to express it as positive. Show calculation set-up and round off the answer to correct sig figs. Answers without proof of calculations will receive no credit. 1. (2 pts) Calculate the density of O₂ gas using the ideal gas law (d = PM/RT) at a) STP conditions b) 1 atm pressure and temperature of 22.5 °C. c) What is/are the main factor(s) that affect(s) the density of O₂ gas in (a) and (b). Why? Be sure to provide all calculation set ups. 2. (2 pts) In this study, the magnesium metal ribbon was dissolved in hydrochloric acid, a monoprotic acid, to produce H₂ gas. If phosphoric acid, a triprotic acid, were used to react with the magnesium rather than hydrochloric acid, does that affect the amount of H₂ gas produced ? In answering this question, first write balanced equations for the reaction of Mg with 1) hydrochloric acid 2) phosphoric acid 1. conditions. a) reaction: H₂ Calculate the molar volume of H, gas under experimental b) -0.421 g Zn x _Lmol Zn Lmol H₂ 0.00644 mol 65.39 g Zn 1 mol Zn Second, the molar volume under experimental conditions is determined by taking the ratio of the volume of H, gas (in L) collected by the n mol H₂. The volume of H, gas is calculated from the total volume collected, taking into account the fact that a small percentage of the total volume is due to the presence of water vapor. By taking the ratio of the P over the P₁, we have the volume fraction of H, gas, which, when multiplied by the total volume, yields the volume of H, gas collected. PPT - Po=769 torr-16.5 torr=752.5 torr First, determine the n mol of H, gas generated by the The molar volume of H, gas under experimental conditions can now be calculated as follows: VH-752.5 torr x 0.156 L-0.153 L 769 torr 0.153 L 0.00644 mol H₂ 2. Calculate the molar volume of H, gas under STP 3. conditions. V₁ 23.8 L/mol Under experimental conditions: Pon = 752.5 torr (= P₁₂) Tor = 19.0°C +273 = 292 K Von Under STP conditions: VSTP Psir TSTP To calculate the molar volume under STP conditions, use the formula of the combined gas law shown below. The accepted value molar volume of an ideal gas is 22.4 L/mol. -0.153 L Calculate the universal gas constant, R. under experimental conditions. = 23.8 L/mol = 1 atm = 760 torr - 0°C -273 K T₁₂ - 292 K -0.00644 mol Use the following formula to calculate R: PHZ-752.5 torr x Latm- 0.990 atm 760 torr LAB ASSIGNMENT In this lab, the following reaction between Mg metal and excess aqueous HCI is being studied: Mg(s) + 2 HCl(aq) MgCl₂(aq) + H₂(g) To start the reaction, a mass of 0.0118 g of Mg is initially added to the reaction vessel. The H₂ gas produced is collected over water. The volume of gas collected is 11.86 mL, and a gas pressure of 776 torr is measured at 23 °C. The vapor pressure of water at 23 °C is 21 torr. Using the above information, answer the questions in the boxed areas beginning on page 4. Question 1: (5 pts) Calculate the molar volume of H₂ gas generated under experimental conditions. Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Question 2 Part A: (5 pts) Calculate the molar volume of H₂ gas generated under STP conditions Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Part B: (0.5 pt) Given that accepted value of molar volume under STP conditions is 22.4 L/mol, calculate the percent error. If the answer is negative, take the absolute value to express it as positive. Show calculation set-up and round off the answer to correct sig figs. Answers without proof of calculations will receive no credit. Question 3 Part A: (5 pts) Calculate the Universal Gas Constant, R, under experimental conditions Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Part B: (0.5 pt) Given that accepted value of the universal gas constant is 0.08206 Lxatm/molxK, calculate the percent error. If the answer is negative, take the absolute value to express it as positive. Show calculation set-up and round off the answer to correct sig figs. Answers without proof of calculations will receive no credit. 1. (2 pts) Calculate the density of O₂ gas using the ideal gas law (d = PM/RT) at a) STP conditions b) 1 atm pressure and temperature of 22.5 °C. c) What is/are the main factor(s) that affect(s) the density of O₂ gas in (a) and (b). Why? Be sure to provide all calculation set ups. 2. (2 pts) In this study, the magnesium metal ribbon was dissolved in hydrochloric acid, a monoprotic acid, to produce H₂ gas. If phosphoric acid, a triprotic acid, were used to react with the magnesium rather than hydrochloric acid, does that affect the amount of H₂ gas produced ? In answering this question, first write balanced equations for the reaction of Mg with 1) hydrochloric acid 2) phosphoric acid 1. conditions. a) reaction: H₂ Calculate the molar volume of H, gas under experimental b) -0.421 g Zn x _Lmol Zn Lmol H, 0.00644 mol 65.39 g Zn 1 mol Zn Second, the molar volume under experimental conditions is determined by taking the ratio of the volume of H, gas (in L) collected by the n mol H₂. The volume of H, gas is calculated from the total volume collected, taking into account the fact that a small percentage of the total volume is due to the presence of water vapor. By taking the ratio of the P over the P₁, we have the volume fraction of H, gas, which, when multiplied by the total volume, yields the volume of H, gas collected. PPT - Po=769 torr-16.5 torr=752.5 torr First, determine the n mol of H, gas generated by the The molar volume of H, gas under experimental conditions can now be calculated as follows: VH-752.5 torr x 0.156 L-0.153 L 769 torr 0.153 L 0.00644 mol H₂ 2. Calculate the molar volume of H, gas under STP 3. conditions. V₁ 23.8 L/mol Under experimental conditions: Pon = 752.5 torr (= P₁₂) Tor = 19.0°C +273 = 292 K Von Under STP conditions: VSTP Psir TSTP To calculate the molar volume under STP conditions, use the formula of the combined gas law shown below. The accepted value molar volume of an ideal gas is 22.4 L/mol. -0.153 L Calculate the universal gas constant, R. under experimental conditions. = 23.8 L/mol = 1 atm = 760 torr - 0°C -273 K T₁₂ - 292 K -0.00644 mol Use the following formula to calculate R: PHZ-752.5 torr x Latm- 0.990 atm 760 torr LAB ASSIGNMENT In this lab, the following reaction between Mg metal and excess aqueous HCI is being studied: Mg(s) + 2 HCl(aq) MgCl₂(aq) + H₂(g) To start the reaction, a mass of 0.0118 g of Mg is initially added to the reaction vessel. The H₂ gas produced is collected over water. The volume of gas collected is 11.86 mL, and a gas pressure of 776 torr is measured at 23 °C. The vapor pressure of water at 23 °C is 21 torr. Using the above information, answer the questions in the boxed areas beginning on page 4. Question 1: (5 pts) Calculate the molar volume of H₂ gas generated under experimental conditions. Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Question 2 Part A: (5 pts) Calculate the molar volume of H₂ gas generated under STP conditions Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Part B: (0.5 pt) Given that accepted value of molar volume under STP conditions is 22.4 L/mol, calculate the percent error. If the answer is negative, take the absolute value to express it as positive. Show calculation set-up and round off the answer to correct sig figs. Answers without proof of calculations will receive no credit. Question 3 Part A: (5 pts) Calculate the Universal Gas Constant, R, under experimental conditions Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Part B: (0.5 pt) Given that accepted value of the universal gas constant is 0.08206 Lxatm/molxK, calculate the percent error. If the answer is negative, take the absolute value to express it as positive. Show calculation set-up and round off the answer to correct sig figs. Answers without proof of calculations will receive no credit. 1. (2 pts) Calculate the density of O₂ gas using the ideal gas law (d = PM/RT) at a) STP conditions b) 1 atm pressure and temperature of 22.5 °C. c) What is/are the main factor(s) that affect(s) the density of O₂ gas in (a) and (b). Why? Be sure to provide all calculation set ups. 2. (2 pts) In this study, the magnesium metal ribbon was dissolved in hydrochloric acid, a monoprotic acid, to produce H₂ gas. If phosphoric acid, a triprotic acid, were used to react with the magnesium rather than hydrochloric acid, does that affect the amount of H₂ gas produced ? In answering this question, first write balanced equations for the reaction of Mg with 1) hydrochloric acid 2) phosphoric acid 1. conditions. a) reaction: H₂ Calculate the molar volume of H, gas under experimental b) -0.421 g Zn x _Lmol Zn Lmol H₂ 0.00644 mol 65.39 g Zn 1 mol Zn Second, the molar volume under experimental conditions is determined by taking the ratio of the volume of H, gas (in L) collected by the n mol H₂. The volume of H, gas is calculated from the total volume collected, taking into account the fact that a small percentage of the total volume is due to the presence of water vapor. By taking the ratio of the P over the P₁, we have the volume fraction of H, gas, which, when multiplied by the total volume, yields the volume of H, gas collected. PPT - Po=769 torr-16.5 torr=752.5 torr First, determine the n mol of H, gas generated by the The molar volume of H, gas under experimental conditions can now be calculated as follows: VH-752.5 torr x 0.156 L-0.153 L 769 torr 0.153 L 0.00644 mol H₂ 2. Calculate the molar volume of H, gas under STP 3. conditions. V₁ 23.8 L/mol Under experimental conditions: Pon = 752.5 torr (= P₁₂) Tor = 19.0°C +273 = 292 K Von Under STP conditions: VSTP Psir TSTP To calculate the molar volume under STP conditions, use the formula of the combined gas law shown below. The accepted value molar volume of an ideal gas is 22.4 L/mol. -0.153 L Calculate the universal gas constant, R. under experimental conditions. = 23.8 L/mol = 1 atm = 760 torr - 0°C -273 K T₁₂ - 292 K -0.00644 mol Use the following formula to calculate R: PHZ-752.5 torr x Latm- 0.990 atm 760 torr LAB ASSIGNMENT In this lab, the following reaction between Mg metal and excess aqueous HCI is being studied: Mg(s) + 2 HCl(aq) MgCl₂(aq) + H₂(g) To start the reaction, a mass of 0.0118 g of Mg is initially added to the reaction vessel. The H₂ gas produced is collected over water. The volume of gas collected is 11.86 mL, and a gas pressure of 776 torr is measured at 23 °C. The vapor pressure of water at 23 °C is 21 torr. Using the above information, answer the questions in the boxed areas beginning on page 4. Question 1: (5 pts) Calculate the molar volume of H₂ gas generated under experimental conditions. Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Question 2 Part A: (5 pts) Calculate the molar volume of H₂ gas generated under STP conditions Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Part B: (0.5 pt) Given that accepted value of molar volume under STP conditions is 22.4 L/mol, calculate the percent error. If the answer is negative, take the absolute value to express it as positive. Show calculation set-up and round off the answer to correct sig figs. Answers without proof of calculations will receive no credit. Question 3 Part A: (5 pts) Calculate the Universal Gas Constant, R, under experimental conditions Show all calculation set-ups leading to the answer for credit. For full credit, all numerical answers must be rounded off to correct sig figs and with proper units. Answers without proof of calculations will receive no credit. Part B: (0.5 pt) Given that accepted value of the universal gas constant is 0.08206 Lxatm/molxK, calculate the percent error. If the answer is negative, take the absolute value to express it as positive. Show calculation set-up and round off the answer to correct sig figs. Answers without proof of calculations will receive no credit. 1. (2 pts) Calculate the density of O₂ gas using the ideal gas law (d = PM/RT) at a) STP conditions b) 1 atm pressure and temperature of 22.5 °C. c) What is/are the main factor(s) that affect(s) the density of O₂ gas in (a) and (b). Why? Be sure to provide all calculation set ups. 2. (2 pts) In this study, the magnesium metal ribbon was dissolved in hydrochloric acid, a monoprotic acid, to produce H₂ gas. If phosphoric acid, a triprotic acid, were used to react with the magnesium rather than hydrochloric acid, does that affect the amount of H₂ gas produced ? In answering this question, first write balanced equations for the reaction of Mg with 1) hydrochloric acid 2) phosphoric acid

Answer rating: 100% (QA)

Using the combined gas law P1V1T1P2V2T2 where subscripts 1 and 2 ref... View the full answer