1) The Lewis structure will be:
Xe
|
I--I
In this structure, the xenon atom is surrounded by two iodine atoms, which are bonded to it through single bonds. Each iodine atom has one lone pair of electrons, for a total of 2 lone pairs on the central atom (xenon).
2) The molar mass of the gaseous compound is 0.416 g/mol.
To draw a correct Lewis structure for XeI2, we need to first count the number of valence electrons in the molecule. Xenon is a noble gas and has 8 valence electrons, while iodine has 7 valence electrons for a total of 23 valence electrons. To satisfy the octet rule and put a 0 formal charge on all atoms, we can use the following Lewis structure:
Xe
|
I--I
To find the molar mass of the gaseous compound, we can use the ideal gas law:
M = dRT/P
Where M is the molar mass, d is the density, R is the ideal gas constant, T is the temperature, and P is the pressure.
Given that the density of the gas is 0.3876 grams/142 mL = 0.002736 grams/mL, the temperature is 150 + 273 = 423 K, the pressure is 775 torr = 775/760 atm = 1.0132 atm, and the ideal gas constant is 0.08206 L·atm/mol·K.
We can calculate the molar mass as follows:
M = (0.002736 g/mL) * (0.08206 L·atm/mol·K / (1.0132 atm)) * (423 K)
M = 0.416 g/mol
Learn more about molar mass, here brainly.com/question/12127540
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