The molar mass of two equally sized samples of unknown gaseous compounds is shown in the table. molar mass comparison gas molar mass a 4.00 g/mol b 2.01 g/mol which statement describes the density and effusion of both gases at stp? gas a has a higher density and effuses faster than gas b. gas a has a higher density and effuses slower than gas b. gas a has a lower density and effuses faster than gas b. gas a has a lower density and effuses slower than gas b.

B. Gas A has a higher density and effuses slower than Gas B

Explanation: To calculate the rate of effusion of gas, we use Graham's Law.

This law states that the rate of effusion of gas is inversely proportional to the square root of the molar mass of the gas. The equation given by this law follows:

For the rate of effusion of A to B, we write the expression:

Thus Gas B would diffuse faster than gas A.

As the two gases are equally sized, the y have same volume but Gas A has higher mass. Thus Gas A would be more dense than Gas B.

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer