rate of reactions Flashcards
what is an anomalous result
a measurement or reading that does not fit in with the pattern of the other results; such a result is not necessarily wrong, but it should be checked
collision
what happens when two or more objects bump into each other
gradient
the steepness of a slope, including on a graph, indicates how fast a reaction has taken place
rate of reaction
how quickly or slowly a reaction happens
rate of reaction equation
rate of reaction = amount of product formed or reactant used up/time
what is the units for rate of reaction
volume - cm3/s
mass - g/s
what is the equation for gradient
rise/run
what is a tangent line
line that touches the curve
what things effect the rate of reaction?
(4)
- surface area
- temperature
- concentration
- pressure
how can you measure the rate of reaction
by working out how much of one of the products has been made in a given time, or how much of a reactant has been used up in a given time
concentration
a measure of how many particles of a substance are in a fixed volume of a solution
dilute
adding water to a solution dilutes it; there are fewer particles of the solute in a fixed volume of the solution
surface area
measurement of the space on the surface of an object measured in cm2
why do smaller pieces of solids (powdered) react faster then lumps of the same mass
they have a larger surface area
precipitate
an insoluble solid formed when two soluble substances react
preliminary work
some practical work you do before an investigation to find out how you will carry it out. for example, you might find out the range or interval of the independent variable that you will use
what is collision theory and what is another name for it
another name for it is particle theory, Collision theory states that for a chemical reaction to occur, the reacting particles must collide with one another. The rate of the reaction depends on the frequency of collisions.
what type of energy does heat give particles
kinetic energy
what is activation energy
the relatively small amount of energy needed to start a chemical reaction
