Hey sample of helium occupies 235 ml at 788 tour and 25°c. if the sample is condensed into a 0.115 l flask what will be the new pressure assuming constant temperature?

The new pressure of helium gas assuming constant temperature is equal to 1610.26 Torr.

Given the following data:

Conversion:

Initial volume = 235 mL to L =

To determine the new pressure assuming constant temperature, we would apply Boyle's law:

Mathematically, Boyle's law is given by the formula;

Where;

Substituting the given parameters into the formula, we have;

Find more information: link

the system is in constant temperature

so it follows Boyle's law

i.e.P1V1=P2P2

where P1=initial pressure=788 tour

P2=final pressure= ?

V1=initial volume=235 ml

V2=final volume=0.115 ml

"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"

jjj89t'ji; it hink the answer is your mom is not si