Calculate the theoretical yield of H2 gas assuming that a 0.5 g sample of Mg is...
- Calculate the theoretical yield of H2 gas assuming that a 0.5 g sample of Mg is completely reacted with each acid. The ideal gas law, PV=nRT, can be used for this calculation, where P=pressure; V=volume; n=amount of substance; R= ideal gas constant; and T= temperature. Assume that pressure is 1 atm and the temperature is room temperature (about 293 K).
Calculate the following ratios for each acid:
for HCl Mole(s) H2Mole of Mg= ______________
for H2SO4 Mole(s) H2Mole of Mg= ______________
- Based on the above ratios, which acid is more efficient at producing H2 gas?
- Why is one acid more efficient than the other? Explain.
- Suppose you were seeking to produce H2 gas as part of a commercial enterprise and you wanted to use the most cost efficient method for produce H2 gas. If the price of a high grade sulfuric acid is $89.00 for 2.5 L and that of HCl is $77.00 for 2.5 L, which acid would be more cost efficient for H2 production?
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Calculate the theoretical yield of H2 gas assuming
that a 0.5 g sample of Mg is...
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2...
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2 + H2 Use the following reaction information to answer the subsequent questions. Show all of your work. 92 mm Length of Magnesium ribbon: Barometric Pressure: 762.9 mmHg Water Temperature: 29 °C Initial Gas Volume: 0.00 mL Final Gas Volume: 67.35 mL 0.7559 Mass = Length (in mm) x (1000 mm) 1. Magnesium is usually found in the laboratory as a ribbon strip. Find the...
Mg(s) + 2 HCl(aq) H2(g) + MgCl2(aq) (2) This problem to be done with Gas Laws...
Mg(s) + 2 HCl(aq) H2(g) + MgCl2(aq) (2) This problem to be done with Gas Laws Chapter. You'll need PV=nRT. You are asked to produce exactly 40.0 mL of H2 gas from the reaction of magnesium and HCl. Using the balanced chemical reaction above, (2), determine how much magnesium (in g) and how much HCl (in mL, assuming you have a 1.0 M solution) you need to add to produce exactly 40.0 mL of H2 gas. Include assumptions you make...
Experiment 12. Generating Hydrogen Cas A. Percent yield of hydrogen gas Mass of magnesium -0.051 Volume...
Experiment 12. Generating Hydrogen Cas A. Percent yield of hydrogen gas Mass of magnesium -0.051 Volume of gas (actual) Temperature of H gas Atmospheric pressure (see barometer) 20 °C 24 mmHg 26PmHg mmHg Vapor pressure of water there mmtig Partial pressure of He gas Calculate the moles of hydrogen gas that should have been produced, starting with the mass of Mg and using the balanced equation. Mg (8) + 2 HCI (aq) → MgCl(aq) + H2 (8) 0.08ling Imoling ....
Mg metal reacts with HCl to produce hydrogen gas. Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) How many grams of magnesium are...
Mg metal reacts with HCl to produce hydrogen gas. Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) How many grams of magnesium are needed to prepare 6.90 L of H2 at 775 mmHg and 20 ∘C?
You have the following reaction: Mg(s) + 2 HCl(aq) + Mg2+(aq) + H2(g) + 2Cl(aq). Answer...
You have the following reaction: Mg(s) + 2 HCl(aq) + Mg2+(aq) + H2(g) + 2Cl(aq). Answer the following questions with the data given. The hydrogen gas is collected above the aqueous acid solution in an inverted graduated cylinder. Moles of Mg metal: Temperature of gas Atmospheric pressure: 0.0033mol 28.0°C 1.02 atm. 3. What is the pressure of the hydrogen gas in the graduated cylinder?
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip...
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip of magnesium metal with 4.00 mL of 4.0 M hydrochloric acid and collected the hydrogen gas produced using the experimental setup you see at the station. Unfortunately, the student forgot to record the mass of the metal before they reacted it with acid. Determine the mass of the magnesium metal the student used in the experiment. For this experiment assume the pressure of the...
in the reaction assume that you added 2.43 g of Mg (s) to the reaction flask and how the reaction goes fully to completi...
in
the reaction assume that you added 2.43 g of Mg (s) to the reaction
flask and how the reaction goes fully to completion
Mg(s) + 2HCl(aq) + MgCl(aq) + H2(B) In the above reaction, assume that you added 2.43 grams of Mg(s) to the reaction flask and the reaction goes fully to completion. a. What is the theoretical weight in grams of MgCl(s) that can be produced ? (2.5 Points) (Show calculations) b. What is the weight in grams...
0.5 points QUESTION 3 Save Answer Zinc reacts with aqueous sulfuric acid to form hydrogen gas:...
0.5 points QUESTION 3 Save Answer Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s)H2SO4 (aq)ZnSO4 (aq) + H2 (g) In an experiment, 225 mL of wet Hp is collected over water at 27 °C with a total pressure of the water-hydrogen mixture of 748 torr. The vapor pressure of water at 27 °C is 26.74 torr How many grams of Zn have been consumed? 431 O 0.567 4.31 x 105 O567 4.79 x 106 0.5 points...
Please answer all questions in both worksheets! Thank you! 1. What is the ideal gas law?...
Please answer all questions in both worksheets! Thank
you!
1. What is the ideal gas law? Write the equation below and label all the components of the equation. 2. Write the balanced chemical equation for the reaction between Mg and HCI below include phases of each constituent. Mg + HCI 3. If a student used an excess of HCl to dissolve 0.045 grams of pure Mg ribbon, and collected the gas in a test tube over water how much H2...
1. Based on the ideal gas law, there is a simple equivalency that exists between the...
1. Based on the ideal gas law, there is a simple equivalency that exists between the amount of gas and the volume it occupies. At standard temperature and pressure (STP; 273.15 K and 1 atm, respectively), one mole of gas occupies 22.4 L of volume. What mass of methanol (CH3OH) could you form if you reacted 3.39 L of a gas mixture (at STP) that contains an equal number of carbon monoxide (CO) and hydrogen gas (H2) molecules? 2. Assuming...
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2 + H2 Use the following reaction information to answer the subsequent questions. Show all of your work. 92 mm Length of Magnesium ribbon: Barometric Pressure: 762.9 mmHg Water Temperature: 29 °C Initial Gas Volume: 0.00 mL Final Gas Volume: 67.35 mL 0.7559 Mass = Length (in mm) x (1000 mm) 1. Magnesium is usually found in the laboratory as a ribbon strip. Find the...
Mg(s) + 2 HCl(aq) H2(g) + MgCl2(aq) (2) This problem to be done with Gas Laws Chapter. You'll need PV=nRT. You are asked to produce exactly 40.0 mL of H2 gas from the reaction of magnesium and HCl. Using the balanced chemical reaction above, (2), determine how much magnesium (in g) and how much HCl (in mL, assuming you have a 1.0 M solution) you need to add to produce exactly 40.0 mL of H2 gas. Include assumptions you make...
Experiment 12. Generating Hydrogen Cas A. Percent yield of hydrogen gas Mass of magnesium -0.051 Volume of gas (actual) Temperature of H gas Atmospheric pressure (see barometer) 20 °C 24 mmHg 26PmHg mmHg Vapor pressure of water there mmtig Partial pressure of He gas Calculate the moles of hydrogen gas that should have been produced, starting with the mass of Mg and using the balanced equation. Mg (8) + 2 HCI (aq) → MgCl(aq) + H2 (8) 0.08ling Imoling ....
You have the following reaction: Mg(s) + 2 HCl(aq) + Mg2+(aq) + H2(g) + 2Cl(aq). Answer the following questions with the data given. The hydrogen gas is collected above the aqueous acid solution in an inverted graduated cylinder. Moles of Mg metal: Temperature of gas Atmospheric pressure: 0.0033mol 28.0°C 1.02 atm. 3. What is the pressure of the hydrogen gas in the graduated cylinder?
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip of magnesium metal with 4.00 mL of 4.0 M hydrochloric acid and collected the hydrogen gas produced using the experimental setup you see at the station. Unfortunately, the student forgot to record the mass of the metal before they reacted it with acid. Determine the mass of the magnesium metal the student used in the experiment. For this experiment assume the pressure of the...
in
the reaction assume that you added 2.43 g of Mg (s) to the reaction
flask and how the reaction goes fully to completion
Mg(s) + 2HCl(aq) + MgCl(aq) + H2(B) In the above reaction, assume that you added 2.43 grams of Mg(s) to the reaction flask and the reaction goes fully to completion. a. What is the theoretical weight in grams of MgCl(s) that can be produced ? (2.5 Points) (Show calculations) b. What is the weight in grams...
0.5 points QUESTION 3 Save Answer Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s)H2SO4 (aq)ZnSO4 (aq) + H2 (g) In an experiment, 225 mL of wet Hp is collected over water at 27 °C with a total pressure of the water-hydrogen mixture of 748 torr. The vapor pressure of water at 27 °C is 26.74 torr How many grams of Zn have been consumed? 431 O 0.567 4.31 x 105 O567 4.79 x 106 0.5 points...
Please answer all questions in both worksheets! Thank
you!
1. What is the ideal gas law? Write the equation below and label all the components of the equation. 2. Write the balanced chemical equation for the reaction between Mg and HCI below include phases of each constituent. Mg + HCI 3. If a student used an excess of HCl to dissolve 0.045 grams of pure Mg ribbon, and collected the gas in a test tube over water how much H2...
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