U10 PT - Kalena Oropeza
Chemical Rates
Reaction rates - how fast reactants turn into products
Reaction Rate = k[A]x(exponent)
k = constant, A = concentration of reactant, x = order of the reaction
Collision Theory - The particles of the reactants must have enough energy and must collide at the proper angle in order for a reaction to occur
Equilibrium
Chemical Equilibrium - when the forward and reverse reactions balance each other because they are taking place at equal rates.
When the concentration of the reactants increases, more molecules or ions interact to form new compounds, and the reaction rate increases as well. When the concentration the reactants decreases, fewer of that molecule or ion is present, and the reaction rate decreases.
If the temperature is increased so is the reaction rate because of the disproportionately large increase in the number of high energy collisions.
Increasing the surface area results in an increased chance of collisions between reactant particles, so there are more collisions and the rate of the reaction increases.
Rate Law - The relationship of the rate of a reaction to the rate constant and the concentrations of the reactants raised to certain powers
rate = k[A]m(exponent)[B]n(exponent)
k = specific rate constant, [A] & [B] = concentrations of reactants A & B, m & n = concentration term exponents ( sum of m & n = reaction order)
Rate Determining Step - the slowest step of a chemical reaction which determines the rate a of a reaction.
[A] & [B] = molar concentrations of the reactants, [C] & [D] = molar concentrations of the products, (a, b, c, d) = coefficients in the balanced equation
Le Châtelier’s Principle: if stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.
Steps to solve(using small x approximation): 1) assume reaction goes 100% to products or reactants
2) ICE table
3) Solve for x, assume x is small
4) Check answer
not enough explanation and results