Question

PLEASE HELP I NEED ASAP.

How many moles of bromine gas would occupy a volume of 20 L at a pressure of .90 atm and a temperature of 90°C? Show all work.
R= 8.31 L kPa/K mol
1 atm-101.3kPa

Answer 1

First, we need to convert the temperature from Celsius to Kelvin by adding 273.15 to it:

90°C + 273.15 = 363.15 K

Then, we can use the Ideal Gas Law to solve for the number of moles:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

We are given P = 0.90 atm, V = 20 L, and T = 363.15 K. We also need to convert the pressure from atm to kPa:

0.90 atm × 101.3 kPa/atm = 91.17 kPa

Substituting these values into the Ideal Gas Law equation and solving for n, we get:

n = PV/RT = (91.17 kPa)(20 L)/(8.31 L kPa/K mol)(363.15 K) = 0.0815 mol

Therefore, the number of moles of bromine gas that would occupy a volume of 20 L at a pressure of 0.90 atm and a temperature of 90°C is 0.0815 mol.

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