Amixture of gases contains methane, ch4, ethane, c2h6, and propane, c3h8. if the total pressure is 1.5 atm and the number of moles of the gases present is .31 mole for methane, .25 mole for ethane, and .29 mole for propane, calculate the partial pressure for the gases.

The partial pressure  for the gases is as below

CH₄=0.547  atm

C₂H₆= 0.441 atm

C₃H₈ =0.512 atm

calculation

 partial  pressure of a  gas=[ (moles  of the gas/ total   moles) x  total pressure]

Total  moles = moles of (  CH₄ + C₂H₆ + C₃H₈)  =0.31 + 0.25 +0.29 = 0.85  moles

Total pressure = 1.5 atm

partial pressure  for CH₄ = (0.31/0.85)  x 1.5 atm=0.547 atm

Partial  pressure for C₂H₆ =( 0.25 /0.85)  x 1.5 atm = 0.441 atm

partial  pressure for C₃H₈ =(0.29/0.85)  x 1.5 atm =0.512 atm

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.