1. Propane gas (C3H8) burns completely in the presence of oxygen gas (O2) to yield carbon dioxide gas (CO2) and water vapor (H2O). ' Write a balanced equation for this reaction. ' Assuming that all volume measurements occur at the same temperature and pressure, how many liters of oxygen will be required to completely burn 0.700 L of propane gas? ' Assuming that all volume measurements occur at the same temperature and pressure, how many liters of carbon dioxide gas will be produced in the reaction? ' Assuming that all volume measurements occur at the same temperature and pressure, how many lit

Question

Chemistry

Noah Snow

6 January, 01:42

1. Propane gas (C3H8) burns completely in the presence of oxygen gas (O2) to yield carbon dioxide gas (CO2) and water vapor (H2O). ' Write a balanced equation for this reaction. ' Assuming that all volume measurements occur at the same temperature and pressure, how many liters of oxygen will be required to completely burn 0.700 L of propane gas? ' Assuming that all volume measurements occur at the same temperature and pressure, how many liters of carbon dioxide gas will be produced in the reaction? ' Assuming that all volume measurements occur at the same temperature and pressure, how many lit

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Answers (1)

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Camryn Mccormick · Answer 1

1) Balanced equation

C3H8 + 5O2 - > 3 CO2 + 4 H2O

2) 0.700 L C3H8

Given the pressure and temperature do not change, the molar ratio is equivalent to volume ratio

1molC3H8 / 5 mol O2 = > 1 L C3H8 / 5 L O2

0.700 L C3H8 / x L O2 = 1 L C3H8 / 5 L O2 = > x = 0.700 L C3H8 * 5 L O2 / 1 L C3H8

x = 3.500 L O2

3) CO2 produced

1 L C3H8 / 3 L CO2 = 0.700 L C3H8 / x L CO2 = >

x = 0.700 L C3H8 * 3 L CO2 / 1 L C3H8 = 2.100 L CO2

4) Water vapor produced

1) 1 L C3H8 / 4 L H2O = 0.700 LC3H8 / x L H2O = >

x = 0.700 L C3H8 * 4 L H20 / 1 L C3H8 = 2.800 L H2O