The partial pressures of CH 4, N 2, and O 2 in a sample of gas were found to be 183 mmHg, 443 mmHg, and 693 mmHg, respectively. What is the mole fraction of nitrogen?

Mole fraction N₂ = 0.336

Explanation:

Mole fraction of a gas can be determined in order to know the partial pressure of the gas, and the total pressure, in the mixture.

Total pressure in the mixture: Sum of partial pressure from all the gases

Total pressure = 183 mmHg + 443 mmHg + 693 mmHg =1319 mmHg

Mole fraction N₂ = Partial pressure N₂ / Total pressure

443 mmHg / 1319 mmHg = 0.336

Remember that mole fraction does not carry units

The mol fraction of N2 is 0.336

Explanation:

Step 1: Data given

Partial pressure CH4 = 183 mm Hg

Partial pressure N2 = 443 mm Hg

Partial pressure O2 = 693 mm Hg

Step 2: Calculate total pressure

Total pressure = partial pressure CH4 + partial pressure N2 + partial pressure O2

Total pressure = 183 mm Hg + 443 mm Hg + 693 mm Hg

Total pressure = 1319 mm Hg

Step 3: Calculate mol fraction

Mol fraction = partial pressure / total pressure

Mol fraction N2 = 443 mm Hg / 1319 mm Hg

Mol fraction N2 = 0.336

The mol fraction of N2 is 0.336

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.