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25 Cards in this Set
- Front
- Back
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Solution |
Stable homogenous mixture of 2 or more substances |
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Solute |
Substance that gets dissolved |
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Solvent |
Substance that causes the solute to dissolve |
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Concentration |
The amount of solute per solvent (or solution) |
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Molarity equation |
M= moles solute/ liters of solution |
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Molality equation |
m = n of solute / kg of solvent **solvent is normally H2O |
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Mole fraction equation |
Xa = nA / nA + nB Xa = mole A / total moles |
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% by mass equation |
% = gA / gA + gB x 100 |
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Ppm (parts per a million) equation |
Ppm = g solute / g solution × 1,000,000 |
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Colligative property |
Property of a solution that is dependent upon concentration (not type of solute) |
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Freezing point depression |
As a solution becomes more concentrated the freezing point decreases 🔼Tf = Kfm |
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Boiling point elevation definition & equation |
The more concentrated a solution the higher the boiling point 🔼Tb = Kbmi Kb is the constant m is the molality i is the number of ions |
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Completion reaction |
Chemical reaction in which the reactants change to products (the reaction stops when the limiting reactant runs out) Ex. 2Mg + O2 ➡ 2MgO |
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Reversible reaction |
Chemical reaction in which reactants form products but then the products can change back to reactants Ex. N2 + 3H2 ↔ 2NH3 |
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Forward reaction |
Reactants change to products ( left to right ) |
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Reverse reaction |
Products change to reactants (right to left) |
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Equilibrium |
Reversible reaction in which the rate of the forward and reverse reactions are equal |
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When is there more products at equilibrium? |
K > 1 |
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When is there more reactants at equilibrium? |
K < 1 |
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Reaction quotient |
A calculation used to determine if a system has obtained equilibrium Q > K -more products -wait for reverse reaction to occur Q < K - more reactants -wait for forward reaction to occur Q = K - at equilibrium |
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Le Chatelier’s Principle |
If a stress is applied to a system at equilibrium it will shift to accommodate the stress |
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How does concentration effect the shift |
An increase in conc. causes the equilibrium to shift to the other side (a decrease in concentration would shift to the same side) |
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How does pressure effect the shift |
An increase in p shifts to the side with the least gas molecules (moles) |
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How does temp effect the shift |
An increase in temp shifts away from the side with heat + = endothermic reaction - = exothermic reaction |
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