The atomic masses of carbon,nitrogen,and oxyg | vedclass

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(A) According to Graham's Law of Diffusion,the rate of diffusion of a gas is inversely proportional to the square root of its molar mass $(r \propto 1

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Carbon dioxide and nitrous oxide

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(A) According to Graham's Law of Diffusion,the rate of diffusion of a gas is inversely proportional to the square root of its molar mass $(r \propto 1/\sqrt{M})$. Therefore,gases with the same molar mass will diffuse at the same rate. The molar mass of $CO_2 = 12 + (2 	imes 16) = 44 \ g/mol$. The molar mass of $N_2O = (2 	imes 14) + 16 = 44 \ g/mol$. Since both $CO_2$ and $N_2O$ have the same molar mass of $44 \ g/mol$,they will diffuse at the same rate.

The atomic masses of carbon,nitrogen,and oxygen are $12, 14$,and $16$ respectively. Which of the following pairs of gases will diffuse at the same rate?

Similar Questions

The gaseous state is characterized by which of the following properties?

The unit of pressure is equivalent to which of the following?

$3.2 \, g$ of oxygen gas diffuses in $10 \, minute$. Under similar conditions,$2.8 \, g$ of nitrogen gas will diffuse in ............ $minute$.

The $\%$ composition by volume of $Cl_2, H_2$,and $N_2$ are in $1:2:7$ by proportion. If the total pressure is $40 \ bar$,find the partial pressures of each gas?
[ Partial pressure $= \frac{\text{Volume } \% \times \text{Total pressure}}{100} ]$

Between $NH_3$ and $CO_2$,which one will diffuse faster? What will be the ratio of their rates of diffusion?

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