# Chem chap 2

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2018-01-29 18:51

## Section

Question | Answer |
---|---|

D[A] | change in concentration of A over time period Dt |

D[B] | change in concentration of B over time period Dt |

when is the rate negative | for A |

rate of A | - (DA/Dt) |

rate of B | DB/Dt |

why is DA negative | because A decreases with time |

average rate | - D[A]/Dt which means D[A]final - D[A]initial/t final - t initial |

rate constant | (K) is rate/D[A] |

What does pV=nRT stand for | P is the pressure of the gas, V is the volume of the gas, n is the amount of substance of gas (in moles), R is the universal gas constant, equal to the product of the Boltzmann constant and the Avogadro constant., T is the temperature of the gas (in Kelvin |

universal gas constant | R is 8.3144598(48) J⋅mol^−1⋅K^−1 |

the ideal gas equation | PV=nRT |

rate of aA+bB=cC | -(1/a)*(D[A]/Dt)=-1/b (DB/Dt)=1/c (DC/Dt) (note: rates on the left side of reaction are negative |

Write the rate expression for the following reaction, CH4 (g) + 2O2 (g) > CO2 (g) + 2H2O (g) | rate = -(D[CH4] / Dt)=-1/2 (D[O2] / Dt)=D[CO2]/Dt=1/2 (D[H2O] / Dt) |

rate law equation | Rate=k [A]^x [B]^y |

according to the rate law, what is the rate of F2 (g) + 2ClO2 (g) > 2FClO2 (g) | rate=k [F2][ClO2 |

how is rate law always determined | experimentally |

how is reaction order always defined | in terms of reactant (not product) concentrations |

is the order of a reactant related to the stoichiometric coefficient of the reactant in the balanced chemical equation | no |

what happens when the concentration doubles | the rate doubles so m=1 |

m | molality=moles of solute / kilograms of solvent |

g to m is | g/molar mass |

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