Starter for five Write the equation showing the relationship between density, mass and volume. Write the equation showing the relationship between density,

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Presentation transcript:

Starter for five Write the equation showing the relationship between density, mass and volume. Write the equation showing the relationship between density, molar mass and molar volume. What is the relationship between all gases at the same temperature and pressure?

Starter for five answers Density = mass ÷ volume Density = molar mass ÷ molar volume At the same temperature and pressure all gases have the same molar volume.

Higher Chemistry Unit 1(e) Gas densities and molar volumes

After today’s lesson you should be able to: Use the two relationships learnt in the last lesson to calculate either the molar mass, molar volume or density of a gas given relevant information. Use the molar mass calculated to identify the unknown gas.

Example 1 A 25cm 3 sample of a gas weighs g and has a molar volume of 29.4l. Calculate its molar mass. Pick out information from question: v = 25cm 3 = 0.025l, m = g and mv = 29.4l Apply to equations: density = mass ÷ volume = ÷ = 0.884g l-1 molar mass = density x molar volume = x 29.4 = 26.0g mass densityvolume molar mass density molar volume

Example 2 A molar volume of CO 2 at standard temperature and pressure is 22.4l. Calculate the mass of a 50cm 3 of the gas under these conditions. Pick out information from question: v = 50cm 3 = 0.050l and mv = 22.4l Apply to equations: density = molar mass ÷ molar volume = 44 ÷ 22.4 = 1.964gl -1 mass = density x volume = x 0.05 = 0.098g mass densityvolume molar mass density molar volume

Example 3 The molar mass of a gas is calculated to be 40g. Identify this gas. First check the molar mass of the monatomic gases on the Periodic Table to see if any have this molar mass. Argon has a molar mass of 40g therefore this gas is Argon. If this was not the case you would then check the molar mass of the diatomic gases to see if they match.

Exercise Complete Q8.11 – 8.25 on p of ‘Test your Higher Chemistry Calculations’. 5 – 10 of these questions will be sufficient.