what is the square root of the gram molecular weight of O2 and CO2, (hint: periodic table) and which one will diffuse faster?
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The reaction of equation would be the following:
1/2(M1)(V^2)1=1/2(M2)(V^2)2
Sqrt*(M1/M2)=V2/V1
The lighter one will diffuse faster, I believe. But check that by reading about Grams law of effusion, I think.
To find the square root of the gram molecular weight of O2 (oxygen) and CO2 (carbon dioxide), we need to know the molecular weights of these compounds.
The molecular weight of an element or compound is the sum of the atomic weights of its constituent elements. We can find the atomic weights of oxygen (O) and carbon (C) on the periodic table.
The atomic weight of oxygen (O) is approximately 16 grams/mol, and the molecular formula for oxygen gas (O2) indicates that it consists of two oxygen atoms. Therefore, the gram molecular weight (molecular weight in grams/mol) of O2 is 2 x 16 = 32 grams/mol.
The atomic weight of carbon (C) is approximately 12 grams/mol, and the molecular formula for carbon dioxide (CO2) indicates that it consists of one carbon atom and two oxygen atoms. Therefore, the gram molecular weight of CO2 is 1 x 12 (carbon) + 2 x 16 (oxygen) = 44 grams/mol.
Now, let's find the square roots of these molecular weights:
Square root of the gram molecular weight of O2 = √32 ≈ 5.657 grams/mol
Square root of the gram molecular weight of CO2 = √44 ≈ 6.633 grams/mol
To determine which gas will diffuse faster, we can use Graham's law of effusion, which states that the rate of effusion or diffusion of a gas is inversely proportional to the square root of its molecular weight.
Therefore, the gas with the smaller molecular weight will diffuse faster. In this case, since O2 has a smaller molecular weight (32 grams/mol) compared to CO2 (44 grams/mol), O2 will diffuse faster than CO2.