A balloon contains a mixture of 2 gases, X and Y. If the pressure in the balloon is 1.50 atm and there are 3 moles of X and 7 moles of Y present, what is the partial pressure of each gas?

Partial Pressure of X = 0.45 atm

Partial Pressure of Y = 1.05 atm

Explanation:

Mixture of gas = Gas X + Gas Y

Total number of moles = 3 + 7 = 10 moles

Total pressure = 1.50 atm

The relationship between partial pressure, total pressure and number of moles is given as;

Partial pressure of gas X  /  Total pressure = Number of moles of gas X  /  Total number of moles

Partial Pressure of gas X  / 1.50 = 3 / 10

Partial Pressure of gas X = 1.5 * 3 / 10 = 0.45 atm

The total pressure of a mixture is a sum total of the individual pressures, hence;

Pressure of mixture = Partial Pressure of X  +   Partial pressure of Y

1.5 = 0.45 +  Partial pressure of Y

Partial Pressure of Y = 1.5 - 0.45 = 1.05 atm

< > according to newton's third law of motion, forces always act in equal but opposite pairs. another way of saying this is for every action, there is an equal but opposite reaction.< >

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.