# An #8 L# container holds #8 # mol and #9 # mol of gasses A and B, respectively. Every two molecules of gas B bind to one molecule of gas A and the reaction raises the temperature from #370^oK# to #425 ^oK#. How much does the pressure change by?

##### 1 Answer

30.377atm at 370K

34.8925atm at 425K

#### Explanation:

So first we need to know the moles of gas

So this is chemistry stoichiometry

So the reagent in excess is A and some amount of it will remain till the end

So if

x = 4.5mol of

Since

So the amount of AB2 is equal to the amount of A used

So A used is 4.5mol

But left out is 8 - 4.5 = 3.5mol

So mol of A + mol of AB2 =

4.5mol + 3.5mol = 8mol

Now calculate the volume of gas at 370K and 425K

using the formula

Where P is pressure in atm

n is moles

R is the universal gas constant which is equal to 0.0821L

T is temperature in kelvin

V is volume

Plug in the variables

Now calculate the pressure at different temperature