Introduction RocketCat sez Propellant is the crap you chuck out the exhaust pipe to make rocket thrust. It's Newton's Law of Action and Reactionsavvy? Fuel is what you burn to get the energy to chuck crap out the exhaust pipe.
This frequently causes problems! The graph below show typical changes in concentration or amount of moles remaining of a reactant with time, for zero, 1st and 2nd order. In the zero order graph the gradient is constant as the rate is independent of concentration, so the graph is of a linear descent in concentration of reactant.
The 2nd order graph tends to 'decay' more steeply than 1st order BUT that proves nothing! The idea is that somehow you test for the order with an appropriate linear graph Connect the graphs with the following: Some possible graphical results are shown above.
Of course  to  could simply represent inaccurate data! There is another graphical way of showing the order with respect to a reactant is 1st order, but it requires accurate data showing how the concentration or moles remaining of a reactant changes with time within a single experiment apart from repeats to confirm the pattern.
The rate of radioactive decay is an example of 1st order kinetics. The graph below shows what happens to a reactant with a half—life of 5 minutes. It is the constancy of the half—life which proves the 1st order kinetics.
The mathematics of 1st order rate equations units. So simplified rate data questions and their solution is given below. So simplified rate data questions and their solutions avoiding graphical analysis are given below. These examples do NOT involve graphs directly, but a 'graphical' section of examples has been added in section 5.
I've made the numbers quite simple to follow the logic of the argument. I've also shown how to calculate the rate constant.
These example calculations below are based on the initial rate of reaction analysis - so we are assuming the variation of concentration with time for each experimental run has been processed in some way e. The graph on the left illustrates the initial rate method for the formation of product.
The gradients A and B would be for two different concentrations of a reactant, the concentration for A would be greater than the concentration of B. The initial rate is taken as the positive tangent - gradient for the curve at the point 0,0. The same argument applies if you imagine the graph inverted and you were following the depletion of a reactant.
Then you would get two negative gradients one steeper than the other for the greater concentration.
Reminder [x] means concentration of x, usually mol dm-3 Example 1. The table below gives some initial data for the reaction:Equation () is the integrated rate law corresponding to the differential rate law given in Eq.
(). While the differential rate law describes the rate of . e has always bothered me — not the letter, but the mathematical constant. What does it really mean?
Math books and even my beloved Wikipedia describe e using obtuse jargon: The mathematical constant e is the base of the natural logarithm. And when you look up the natural logarithm you get: The. The Arrhenius equation. Rate constants and rate equations.
In the equation, we have to write that as J mol The value of the gas constant, R, is J K-1 mol The catalyst is bound to be involved in the slow step of the reaction, and a new rate equation will have to include a term relating to the catalyst.
Recreational mathematics by Dr. Gerard P. Michon. Fun questions can help demonstrate useful mathematical tools. Classic puzzles and riddles. Propellant is the crap you chuck out the exhaust pipe to make rocket thrust. It's Newton's Law of Action and Reaction, savvy?Fuel is what you burn to get the energy to chuck crap out the exhaust pipe.
Apr 19, · Chemistry question need help pleasee? ashio-midori.com effect does concentration have on reaction rate? ashio-midori.com the mathematical equation used to determine the average rate of a chemical ashio-midori.com: Resolved.