A sample of ideal gas is heated in a 2L vessel at a temperature of 320 Kelvin. the pressure in the vessel is 2.5 atm. What is the new pressure in the vessel if the volume is halved and the temperature is reduced to 250 Kelvin?

Pressure=3.91atm

Explanation:

As given in the question that gas is ideal so

we can use Ideal gas equation

volume of gas is not given directly but volume of container is given and we know gas takes the volume in which they are kept.

therefore  mole remains contant

P1=2.5 atm

V1=2L

T1=320K

P1=?

V1=1L

T1=250K

..............(1)

................(2)

eqn2/eqn1

Pressure=3.91atm

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"