 # Chem chap 2 rename version from 2018-01-29 18:51 edit

## Section

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 negativefor A
rate of A- (DA/Dt)
rate of BDB/Dt
why is DA negativebecause 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 forP 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 constantR is 8.3144598(48) J⋅mol^−1⋅K^−1
the ideal gas equationPV=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 equationRate=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 determinedexperimentally
how is reaction order always definedin terms of reactant (not product) concentrations
is the order of a reactant related to the stoichiometric coefficient of the reactant in the balanced chemical equationno
what happens when the concentration doublesthe rate doubles so m=1
mmolality=moles of solute / kilograms of solvent
g to m isg/molar mass