Understanding Gas Laws: Key Concepts and Calculations in CHEM
School
Auburn University**We aren't endorsed by this school
Course
CHEM 1030
Subject
Chemistry
Date
Dec 11, 2024
Pages
2
Uploaded by ChefWren8414
CHEM 1030 Chapter 10 Recitation Sheet Name:___________________________ Write the three simple gas laws: Charles’s Law Avogadro’s Law Boyle’s Law For each of the following problems, identify which gas law is being used. A sample of gas has a volume of 2.80 L at an unknown temperature. When you submerge the sample in ice water at T= 0.00℃, its volume decreases to 2.57 L. What was its initial temperature in Kelvin? A sample of gas has an initial volume of 12.5 L at a pressure of 1.25 atm. If the sample is compressed to a volume of 3.2 L, what is its pressure? What is the ideal gas law? Write the equation Write the gas constant which will be used for CHEM 1030. (Do not forget units!) A container with a volume of 65 L contains NH3at 0.9 atm and 30°C. How many moles of gas are present? What mass of gas is present? (NH3molar mass = 17 g/mol)
How many grams of water form when 3.2 L of oxygen gas at 298K and 0.1 atm completely reacts with hydrogen gas?2!!(#) + &!(#) → 2!!&(#)a.First, how many moles of oxygen are present in the flask? (Hint: PV=nRT) b.Use the moles of oxygen to calculate how many grams of water will form. (This is a stoichiometry problem similar to Ch. 7 problems…) 2NaBH4(s) + 2H3PO4(l) ®B2H6(g) + 2NaH2PO4(s) + 2H2(g) A reaction of NaBH4and H3PO4creates solid NaH2PO4and two gases, B2H6(27.66 g/mol) and H2(2 g/mol). The flask collecting the gases is at 1 L and the temperature is 350 K. If 0.136 g of H2and 3.4 g B2H6were produced, answer the following. a.How many moles total, nT, (moles B2H6AND H2) are in the flask? b.What is the total pressure in the flask? (PTV=nTRT) c.What is the mole fraction for B2H6? What is the mole fraction for H2? d.What is the partial pressure of B2H6AND H2? (Remember partial pressure is total pressure times mole fraction.) This graph shows the distribution of molecular velocities for the same gas at two different temperatures (A and B). Which temperature is higher? Then, draw a graph of samples of the same gas at different temperatures E, F, and G. Condition G has the lowest temperature and F has the highest temperature. A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. a.Which of the two gases is heavier? b.Which of the two gases exerts the greater partial pressure? c.The molecules or atoms of which gas will have the greater average velocity? d.The molecules of which gas will have the greater average kinetic energy? e.If a small hole were opened in the flask, which gas would effuse more quickly? f.Draw a graph of the distributions of molecular velocities.