A mixture of gases at a total pressure of 725 mmHg contains nitrogen, carbon dioxide, helium, and oxygen. The partial pressure of carbon dioxide is 175 mmHg, the partial pressure of nitrogen is 355 mmHg, and the partial pressure of helium is 15 mmHg. What is the partial pressure of oxygen?

The partial pressure of oxygen is 180 mm Hg

Explanation:

According to Dalton's law, the total pressure is the sum of individual pressures.

Given : =total pressure of gases = 725 mm Hg

= partial pressure of nitrogen  = 355 mm Hg

= partial pressure of carbon dioxide  = 175 mm Hg

= partial pressure of helium  = 15 mm Hg

= partial pressure of oxygen  = ?

putting in the values we get:

The partial pressure of oxygen is 180 mm Hg

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

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