Molecule per liter

This concentration describes a concentration of one thousand molecules per liter. 

Now let us consider the mechanism of the formation of N2O4 molecules by combination of NOo molecules. In order for an NoO molecule to be formed, two NOo molecules must collide tvith one another. The chance that a given molecule of N0.> will collide tvitli another molecule of NOo is obviously proportional to the concentration of NO2 molecules—if the number of NOo molecules per liter is doubled, the chance that a given molecule of NOo wall collide wdth another one will be multiplied by 2. Since the number of collisions experienced by a particular molecule is proportional to [NOo], the total number of collisions experienced by all the molecules in 1 liter of the gas is proportional to the square of this quantity. Accordingly... 

AIM solution contains one Avogadro s number of molecules per liter,... 

In the above, K has been expressed in terms of volume concentrations (gram-molecules per liter) Let us now express it in terms of partial pressures For the partial pressure A of the gas A m the equilibrium state we have—... 

The equilibrium constant here referred to is that defined either m volume concentration terms (gram-molecules per liter) or in terms of partial pressures It has already been shown in the case of a gaseous system that the equilibrium constant defined in either of these two ways is independent of external pressure We are not considering at the moment the third way of defining the equilibnum constant (Planck s form), m which molecular concentrations or molar fractions are employed The latter equilibnum constant, which we have already discussed in the case of gases, varies with the external pressure even in the gaseous case, and, as Planck has shown, vanes likewise in the case of a reaction in solution We are concerned at present, however, with the ordinary equilibrium constant K defined in terms of volume concentrations The considerations apply equally well to the constant defined in terms of partial osmotic pressures... 

On a smoggy day in a certain city the ozone concentration was 0.42 ppm by volume. Calculate the partial pressure of ozone (in atm) and the number of ozone molecules per liter of air if the temperature and pressure were 20.0°C and 748 mmHg, respectively. 

Plan We must find the density (d) and number of molecules of CO2, given the two sets of P and T data. We find M, convert T to kelvins, and calculate d with Equation 5.9. Then we convert the mass per liter to molecules per liter with Avogadro s number. 

Solution (a) Density and molecules per liter of CO2 at STP. Summary of gas properties ... 

At the higher temperature in (b), the density should decrease, which can happen only if there are fewer molecules per liter, so the answer is reasonable. 

The influence of electrolytes upon the distribution of acetic acid between the aqueous and chloroform layers was investigated by Rothmund and Wilsmore, and the following results expressed in gram molecules per liter at 25° were obtained ... 

The allowable concentration level of vinyl chloride, C2H3CI, in the atmosphere in a chemical plant is 2.0 X 10 g/L. How many moles of vinyl chloride in each liter does this represent How many molecules per liter ... 

Consider the following hypothetical reactions. The equilibrium constants K given for each reaction are defined in terms of a concentration unit of molecules per liter. 

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