**Part A: ****Given:**

P = 651 torr = 0.8566 atm

V = 1.00 m^{3} = 1000 L

T = 19 °C + 273 = 292 K

**Calculating for n:**

$\mathbf{n}\mathbf{=}\frac{(0.8566\overline{)\mathrm{atm}})(1000\overline{)L})}{(0.08206{\displaystyle \frac{\overline{)\mathrm{atm}}\xb7\overline{)L}}{\mathrm{mol}\xb7\overline{)K}}})(292\overline{)K})}$** = 35.75 mol dry air**

Part A:

What mass of carbon dioxide is present in 1.00 m3 of dry air at a temperature of 19°C and a pressure of 651torr? Express your answer with the appropriate units.

Part B:

Calculate the mass percentage of oxygen in dry air. Express your answer with the appropriate units.

Here is given info:

Air is a mixture of several gases. The 10 most abundant of these gases are listed here along with their mole fractions and molar masses.

Component | Mole fraction | Molar mass (g/mol) |

Nitrogen | 0.78084 | 28.013 |

Oxygen | 0.20948 | 31.998 |

Argon | 0.00934 | 39.948 |

Carbon dioxide | 0.000375 | 44.0099 |

Neon | 0.00001818 | 20.183 |

Helium | 0.00000524 | 4.003 |

Methane | 0.000002 | 16.043 |

Krypton | 0.00000114 | 83.80 |

Hydrogen | 0.0000005 | 2.0159 |

Nitrous oxide | 0.0000005 | 44.0128 |

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