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With a pressure increase due to a decrease in volume, the side of the equilibrium with fewer moles is more favorable [10] and with a pressure decrease due to an increase in volume, the side with more moles is more favorable. There is no effect on a reaction where the number of moles of gas is the same on each side of the chemical equation.
For a reversible reaction, the equilibrium constant can be measured at a variety of temperatures. This data can be plotted on a graph with ln K eq on the y-axis and 1 / T on the x axis. The data should have a linear relationship, the equation for which can be found by fitting the data using the linear form of the Van 't Hoff equation
The production-possibility frontier can be constructed from the contract curve in an Edgeworth production box diagram of factor intensity. [12] The example used above (which demonstrates increasing opportunity costs, with a curve concave to the origin) is the most common form of PPF. [ 13 ]
is computed by first calculating a residual value ˙, resulting from spurious mass flux, then using this mass imbalance to get a new pressure value. The pressure value that is attempted to compute, is such that when plugged into momentum equations a divergence-free velocity field results. The mass imbalance is often also used for control of the ...
The volume change can thus be understood to be the pressure dependency of the change in Gibbs free energy associated with the reaction. When a single step in a reaction is perturbed in a pressure jump experiment, the reaction follows a single exponential decay function with the reciprocal time constant (1/τ) equal to the sum of the forward and ...
An example PPF: points B, C and D are all productively efficient, but an economy at A would not be, because D involves more production of both goods. Point X cannot be achieved. Productive efficiency occurs under competitive equilibrium at the minimum of average total cost for each good, such as the one shown here.
The commonly known phases solid, liquid and vapor are separated by phase boundaries, i.e. pressure–temperature combinations where two phases can coexist. At the triple point, all three phases can coexist. However, the liquid–vapor boundary terminates in an endpoint at some critical temperature T c and critical pressure p c. This is the ...
At equilibrium, the rate of transfer of CO 2 from the gas to the liquid phase is equal to the rate from liquid to gas. In this case, the equilibrium concentration of CO 2 in the liquid is given by Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. [1]