To determine the molar mass of the unknown gas, we use Graham's Law of Effusion where it relates the effusion rates of two gases with their molar masses. It is expressed as r1/r2 = √M2/M1. We calculate as follows:
Let 1 = argon gas 2 = unknown gas
r2 = 0.91r1r1/r2 = 1/0.91
1/0.91 = √M2/M1 = √M2/40M2 = 48.30 g/mol
Eazy, it’s called density
I’m only in 8th grade science you know
The major shortcoming of Rutherford's model was that it was incomplete. It did not explain how the atom's negatively charged electrons are distributed in the space surrounding its positively charged nucleus. A form of energy that exhibits wavelike behavior as it travels through space.
plz mark me as brainliest :)
Answer:
aa. Which sample(s) is classified as a compound? How do you know?
mass MgCl₂ = mol x MM MgCl₂ = 0.05 x 95.211 g/mol = 4.76 g
mass Cl in MgCl₂ :
= (2 x AM Cl)/MM MgCl₂ x mass MgCl₂
= (2 x 35.5 g/mol)/95.211 g/mol x 4.76
= 3.55 g
% mass Cl in the mixture :
= (mass Cl / mass mixture) x 100%
= 3.55 / 9.8 x 100%
= 36.22%
