You have 49.8 g of o2 gas in a container with twice the volume as one with co2 gas. the pressure and temperature of both containers are the same. calculate the mass of carbon dioxide gas you have in the container.

34.2 g is the mass of carbon dioxide gas one have in the container.

Explanation:

Moles of :-

Mass = 49.8 g

Molar mass of oxygen gas = 32 g/mol

The formula for the calculation of moles is shown below:

Thus,

Since pressure and volume are constant, we can use the Avogadro's law  as:-

Given ,  

V₂ is twice the volume of V₁

V₂ = 2V₁

n₁ = ?

n₂ = 1.55625 mol

Using above equation as:

n₁ = 0.778125 moles

Moles of carbon dioxide = 0.778125 moles

Molar mass of = 44.0 g/mol

Mass of = Moles × Molar mass = 0.778125 × 44.0 g = 34.2 g

34.2 g is the mass of carbon dioxide gas one have in the container.

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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