Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl 2 (aq) + H 2 (g) (a) How many liters of H 2 would be formed at 742 mm Hg and 15 °C if 25.5 g of zinc was allowed to react?

Hey everyone. So we have the following reaction that shows the decomposition of ammonium carbonate and at 28°C and 1.24 atmosphere test to determine the total volume of gas form 15.26 g of ammonium carbonate. That's completely decomposed total total number of malls. He goes to molds of NH three, that's one more Of c. 0. 2. That's one more Of H 20. And this will give us a total of four moles of gas. So now we need to convert from grams of ammonium carbonate, two moles of gas. We have 15.26 grams of ammonia carbonate. And in one mole that the Mueller mass, it's gonna be too. I'm 14.007 g plus eight Times 1.008g as well. 011 g plus three Times 15.999 gramps. Give us 96.086 g. And in one mole of ammonia carbonate, They're four moles of gas. This will give us 0.63 53 balls of gas. So now we can use the ideal gas out to find the total volume. It's going to be PB It goes N R. T. The pressure is 1.24 atmosphere. The volume is what we're looking for Number of moles. 0.6353. Our constant is 0.08 21. There's some atmosphere about about malls. I'm Calvin And the temperature is 28 degrees Celsius. We need to convert our temperature into Calvin 28°C. We need to add 273.15. This will give us 301 15 kelvin. So now we can put the values into the equation and solve for the volume. It's going to give us 1.24 atmosphere terms of volume Equals 0.63 malls From 0.08 later. Sounds atmosphere. What about moles and kelvin? I'm staying in one 15 kelvin. We get 1.24 times of volume. It was 15.707. So if we divide both sides by 1.24, We get a volume of 12.7 L. Thanks for watching my video and I hope it was helpful.

Ch.10 - Gases: Their Properties & Behavior

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McMurry 8th Edition

Ch.10 - Gases: Their Properties & Behavior

Problem 72a

Chapter 10, Problem 72a

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl₂(aq) + H₂(g) (a) How many liters of H₂ would be formed at 742 mm Hg and 15 °C if 25.5 g of zinc was allowed to react?

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Determine the number of moles of zinc (Zn) using its molar mass.

Use the stoichiometry of the balanced chemical equation to find the moles of hydrogen gas (H_2) produced.

Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.

Use the ideal gas law, PV = nRT, to solve for the volume of hydrogen gas (H_2) in liters. Remember to convert pressure from mm Hg to atm by dividing by 760.

Substitute the known values into the ideal gas law equation and solve for the volume of H_2.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. In this case, the balanced equation shows that one mole of zinc reacts with two moles of hydrochloric acid to produce one mole of hydrogen gas. Understanding stoichiometry allows us to determine the amount of hydrogen gas produced from a given mass of zinc.

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the volume of hydrogen gas produced under specific conditions of pressure and temperature. By rearranging the equation, we can solve for volume when the number of moles of hydrogen is known.

Gas Laws and Conditions

Gas laws describe the behavior of gases under various conditions. In this problem, we need to consider the pressure (742 mm Hg) and temperature (15 °C) to find the volume of hydrogen gas produced. Converting temperature to Kelvin and pressure to atmospheres may be necessary to apply the Ideal Gas Law correctly, ensuring accurate calculations.

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What are the molecular weights of the gases with the following densities: (a) 1.342 g/L at STP

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What are the molecular weights of the gases with the following densities: (b) 1.053 g/L at 25 °C and 752 mm Hg

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Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl₂(aq) + H₂(g) (b) How many grams of zinc would you start with if you wanted to prepare 5.00 L of H2 at 350 mm Hg and 30.0 °C?

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Ammonium nitrate can decompose explosively when heated according to the equation 2 NH4NO31s2¡2 N21g2 + 4 H2O1g2 + O21g2 How many liters of gas would be formed at 450 °C and 1.00 atm pressure by explosion of 450 g of NH4NO3?

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The reaction of sodium peroxide 1Na2O22 with CO2 is used in space vehicles to remove CO2 from the air and generate O2 for breathing:2 Na2O21s2 + 2 CO21g2¡2 Na2CO31s2 + O21g2(a) Assuming that air is breathed at an average rate of 4.50 L/min (25 °C; 735 mm Hg) and that the concentration of CO2 in expelled air is 3.4% by volume, how many grams of CO2 are produced in 24 h?

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl2(aq) + H2(g) (a) How many liters of H2 would be formed at 742 mm Hg and 15 °C if 25.5 g of zinc was allowed to react?

Verified video answer for a similar problem:

Key Concepts

Stoichiometry

Ideal Gas Law

Gas Laws and Conditions

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl₂(aq) + H₂(g) (a) How many liters of H₂ would be formed at 742 mm Hg and 15 °C if 25.5 g of zinc was allowed to react?