Answer :
The molar mass of the compound is 67.5g/mol.
How do you find the molar mass of the compound?
We know that ideal gas law use the formula PV = nRT and can also be written as PM = dRT. Here d refers to the density of the ideal gas law, P refers to the pressure which is measured in atmospheres (atm), T refers to the temperature which is measured in kelvin (K), and R is the ideal gas law constant ,i.e, 0.0821 atm(L)/mol(K) and M is know as the molar mass (g/mol) and d is the density (g/L).
The given details in the question are:-
P = 2.88 atm
d = 7.71g/L
R = 0.0821 atm(L)/mol(K)
T = 36 C = 36+273 = 309 K
M = ?
According to the ideal gas law, we can write the formula to find molar mass as
M = dRT/P
= (7.71*0.0821*309)/2.88
M = 67.83g
∴ Molecular Formula = [tex]ClO_{2}[/tex]
The molar mass of [tex]ClO_{2}[/tex] = 35.5+2*16 = 67.5g.
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The correct question is:
"A chemist has synthesized a greenish-yellow gaseous compound that contains only chlorine and oxygen and has a density of 7. 71 g/l at 36. 0°c and 2188. 8 mmhg. What is the molar mass of the compound?.
Options:
A.[tex]ClO_{3}[/tex]
B.[tex]ClO_{2}[/tex]
C.CIO
D.[tex]Cl_{2}[/tex][tex]O_{2}[/tex]"
