Asample of gas initially has a volume of 859 ml at 565 k and 2.20 atm. what pressure will the sample have if the volume changes to 268 ml while the temperature is increased to 815 k?

We have that the pressure the sample have if the volume changes to 268 ml while the temperature is increased to 815 k is

From the question we are told

A sample of gas initially has a volume of 859 ml at 565 k and 2.20 atm. What pressure will the sample have if the volume changes to 268 ml while the temperature is increased to 815 k

Generally the equation for the ideal gas   is mathematically given as

PV=nRT

Where

Therefore

THEREFORE

the pressure the sample have if the volume changes to 268 ml while the temperature is increased to 815 k is

For more information on this visit

link

10.2 atm

Explanation:

Use ideal gas law:

PV = nRT

Initial number of moles is:

(2.20 atm) (0.859 L) = n (0.0821 atm L / mol / K) (565 K)

n = 0.0407 mol

At the new volume and temperature, the pressure is:

P (0.268 L) = (0.0407 mol) (0.0821 atm L / mol / K) (815 K)

P = 10.2 atm

. west

energy can be converted from one form to another, but it cannot be created or destroyed in ordinary chemical or physical means. do not understand what you are asking but hope this