A sample of N2 gas is contaminated with a gas (A) of unknown molar mass. The partial pressure of each gas is known to be 200 tore at 25 degrees Celsius. The gas are allowed to Effuse through a pinhole, and it is found that has A escapes at 4 times the rate of N2. The molar mass of gas A is:

A. 1.75 g/mol
B. 448 g/mol
C. 112 g/mol
D. 7.01 g/mol
E. None of these

The molar mass of gas A is 1.75 g/mol

Explanation:

To calculate the rate of diffusion of gas, we use Graham's Law.

This law states that the rate of effusion or diffusion of gas is inversely proportional to the square root of the molar mass of the gas. The equation given by this law follows the equation:

So,

We are given:

Molar mass of nitrogen gas = 28 g/mol

Molar mass of A gas = ? g/mol

Putting values in above equation, we get:

Thus molar mass of gas A is 1.75 g/mol

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.