A container holds 6.4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container. If the total pressure is 1.24 atm. What is the partial pressure of hydrogen? Use StartFraction P subscript a over P subscript T EndFraction equals StartFraction n subscript a over n subscript T EndFraction.. 0.31 atm 0.93 atm 5.2 atm 31 atm

0.31 atm

Explanation:

According to the Dalton's law of partial pressure, the total pressure of the gaseous mixture is equal to the sum of the pressure of the individual gases.

Also, the partial pressure of the gas is equal to the product of the mole fraction and total pressure.

Given, for hydrogen gas, it is 25% of the total moles.

So, Mole fraction = 0.25

Total pressure = 1.24 atm

Partial pressure of hydrogen = 0.25 * 1.24 atm = 0.31 atm

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

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