When the pressure changes from 1417 psi to psi the volume changes from 0.145 l to 0.878 l and the temperature changes from 287 k to 196k

When the pressure changes from 1417 psi to  160.186 psi the volume changes from 0.145 L to 0.878 l and the temperature changes from 287 k to 196 k

Explanation:

According to general gas equation:

P₁V₁/T₁ = P₂V₂/T₂

Given data:

Initial volume = 0.145 L

Initial pressure = 1417 psi (1417/14.696 =96.42 atm)

Initial temperature = 287 K

Final temperature = 196 K

Final volume = 0.878 L

Final pressure = ?

Formula:

P₁V₁/T₁ = P₂V₂/T₂

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂  = Final temperature

Solution:

P₂ = P₁V₁ T₂/ T₁ V₂  

P₂ = 96.42 atm × 0.145 L × 196 K / 287 K × 0.878 L

P₂  =  2740.26 atm .L.  K  / 251.99 k. L

P₂  = 10.9 atm

atm to psi:

10.9 × 14.696 = 160.186 psi

"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"

so she was walking and she stepped on warm jeffy , uh uh uhh dadye i just pooped my pants