A chemical reaction conducted in a test tube is suspected of generating oxygen gas. a) Using...

  

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A chemical reaction conducted in a test tube is suspected of generating oxygen gas. a) Using laboratory equipment normally available in a high school classroom, explain how you would collect the gas. b) Describe one test and the subsequent result that could be conducted on the gas to confirm its identity. Nitrogen monoxide, which is present in urban air pollution, immediately converts to nitrogen dioxide as it reacts with oxygen gas. a) Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen monoxide. b) What mole ratio would you use to convert from moles of oxygen gas to moles of nitrogen dioxide? Octane (C&H18) is a fuel component of gasoline. When octane is combusted, carbon dioxide and water vapour are released. a) Write a balanced equation for the reaction. b) The density of gasoline is 0.77 g/cm³. Assuming that the fuel is entirely octane, what mass of carbon dioxide is produced during the complete combustion of 40.0 L of this fuel? c) How many molecules of carbon dioxide were released during the reaction? A chemical reaction conducted in a test tube is suspected of generating oxygen gas. a) Using laboratory equipment normally available in a high school classroom, explain how you would collect the gas. b) Describe one test and the subsequent result that could be conducted on the gas to confirm its identity. Nitrogen monoxide, which is present in urban air pollution, immediately converts to nitrogen dioxide as it reacts with oxygen gas. a) Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen monoxide. b) What mole ratio would you use to convert from moles of oxygen gas to moles of nitrogen dioxide? Octane (C&H18) is a fuel component of gasoline. When octane is combusted, carbon dioxide and water vapour are released. a) Write a balanced equation for the reaction. b) The density of gasoline is 0.77 g/cm³. Assuming that the fuel is entirely octane, what mass of carbon dioxide is produced during the complete combustion of 40.0 L of this fuel? c) How many molecules of carbon dioxide were released during the reaction?