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Mass of oxygen

markosheehan

Member
Jun 6, 2016
136
Calculate the mass of 78 cm3 of oxygen at room temperature and pressure .

Im trying to work out the number of moles and then multiply by 32.
 

Joppy

Well-known member
MHB Math Helper
Mar 17, 2016
259
Calculate the mass of 78 cm3 of oxygen at room temperature and pressure .

Im trying to work out the number of moles and then multiply by 32.
$n(O) = \dfrac{V(O)}{V_m(O)}$

$m(O) = n(O)M(O)$.

$V_m$ is the molar gas volume.
 

markosheehan

Member
Jun 6, 2016
136
Im sorry I am still confused. I know the right answer is .104g
 

Klaas van Aarsen

MHB Seeker
Staff member
Mar 5, 2012
9,491
Im sorry I am still confused. I know the right answer is .104g
The molar volume of a gas ($V_m$) at room temperature and standard pressure is $24$ liter.
That is, $1$ mole is $24$ liter.
How many moles does that make in $78\text{ cm}^3$?
 

markosheehan

Member
Jun 6, 2016
136
Thanks.
I feel the answer is wrong. 78/24000 ×32 is what gives the answer at the back of the book. Should it not be multiplied by 16 though because in the balanced equation for the reaction it's a half mile of oxygen is formed.?
 

Klaas van Aarsen

MHB Seeker
Staff member
Mar 5, 2012
9,491
Thanks.
I feel the answer is wrong. 78/24000 ×32 is what gives the answer at the back of the book. Should it not be multiplied by 16 though because in the balanced equation for the reaction it's a half mile of oxygen is formed.?
Not sure what you mean. Was there a reaction involved?

We have 78/24000 moles of oxygen molecules ($O_2$).
Each molecule consists of 2 oxygen atoms, and an oxygen atom has mass 16u.
Therefore we multiply the moles with $2\times 16=32$.
 

markosheehan

Member
Jun 6, 2016
136
sorry i forgot to mention it was calculate the mass of 78 cm3 of oxygen produced by the the composition of hydrogen peroxide.
h202 goes to h20 +.5o2
so does this not mean you would multiply it by 16 instead of 32