how many grams of bromine will be present in a sample that molar mass of 70.0 g/mol and occupies a 2.00L container at 117 kPa and 35.1C
To determine the number of grams of bromine present in a sample, we need to use the ideal gas law equation, which is given by:
PV = nRT
Where:
P = pressure (in pascals)
V = volume (in liters)
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature (in Kelvin)
First, we need to convert the given conditions to the appropriate units:
Pressure:
117 kPa × (1000 Pa/1 kPa) = 117,000 Pa
Volume:
2.00 L
Temperature:
35.1ºC + 273.15 = 308.25 K
Now, we have all the required values to calculate the number of moles (n), and subsequently, the grams of bromine.
Let's rearrange the ideal gas law equation to solve for n:
n = PV / RT
Substituting the given values:
n = (117,000 Pa) * (2.00 L) / [(8.314 J/(mol·K)) * (308.25 K)]
Calculating this expression will yield the value of n, the number of moles. It is important to note that the moles result is independent of the substance and will represent the number of moles of any gas present in the given conditions.
Once you have the value of n, you can calculate the grams of bromine by using the molar mass of bromine:
grams of bromine = n * molar mass of bromine
Given that the molar mass of bromine is 70.0 g/mol, you can multiply the number of moles (n) by 70.0 g/mol to obtain the answer in grams.