Solve the following, show all work and units for your calculation: Let's say we have a mixture of hydrogen gas
(H2), and oxygen gas (O2). The mixture contains 6.7 mol hydrogen gas and 3.3 mol oxygen gas. The mixture is
in a 300 L container at 273 K and the total pressure of the gas mixture is 0.75 atm. What is the partial
pressure for each gas?

The partial pressure of hydrogen gas is 0.503 atm and that of oxygen gas is 0.248 atm

Explanation:

We are given:

Moles of hydrogen gas = 6.7 moles

Moles of oxygen gas = 3.3 moles

Mole fraction of a substance is given by:

Mole fraction of hydrogen gas,

Mole fraction of oxygen gas,

To calculate the total pressure of the container, we use the equation given by Raoult's law, which is:

where,

= partial pressure of substance

= total pressure

= mole fraction of substance

We are given:

Putting values in above equation, we get:

We are given:

Putting values in above equation, we get:

Hence, the partial pressure of hydrogen gas is 0.503 atm and that of oxygen gas is 0.248 atm

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.