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Weighing gases lab

Weighing gases lab. Results. Gas. Flask. Flask+gas. Mass (g). Density(g/L). H 2. 345.00. 345.08. 0.0835. 0.0835. O 2. 345.00. 346.32. 1.32. 1.32. CO 2. 345.00. 346.82. 1.82. 1.82. Gas. Molar mass (g/mol). Moles (mol). # of molecules. H 2. 2.02. 0.041 3. 2.4 9 x 10 22.

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Weighing gases lab

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  1. Weighing gases lab

  2. Results Gas Flask Flask+gas Mass (g) Density(g/L) H2 345.00 345.08 0.0835 0.0835 O2 345.00 346.32 1.32 1.32 CO2 345.00 346.82 1.82 1.82 Gas Molar mass (g/mol) Moles (mol) # of molecules H2 2.02 0.0413 2.49 x 1022 O2 32.00 0.0413 2.48 x 1022 CO2 44.01 0.0414 2.49 x 1022

  3. O2 H2 • Law of Combining gas volumes: “When measured at the same temp. and pressure, volumes of gaseous reactants and products of chemical reactions are always in simple ratios of whole numbers”. Avogadro's theory: “Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules”. • Yes. All 1 L flasks (same temp & pressure) held the same number of molecules. • O2 molecules are16x more massive (see molar masses): • The mole ratios in the balanced chemical equation.

  4. Mass (g) Density(g/L) Gas Flask Flask +gas H2 345.00 345.08 0.08 O2 345.00 346.32 1.32 CO2 345.00 346.82 1.82 CH4 345.00 345.66 0.66 Molar mass (g/mol) Moles (mol) # of molecules H2 2.02 0.0413 2.49 x 1022 O2 32.00 0.0413 2.48 x 1022 CO2 44.01 0.0414 2.49 x 1022 CH4 16.05 0.0413 2.49 x 1022

  5. +  hydrogen chloride hydrogen chlorine +  carbon monoxide oxygen carbon dioxide +  nitrogen hydrogen ammonia Avogadro’s Theory: Graphical Representation For more lessons, visit www.chalkbored.com

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