The densities of gases A, B, and C at STP are 1.25g/L, 2.87 g/L, and .714 g/L. Calculate the molar mass of each substance. Indentify each substance as ammonia, sulfur dioxide, chlorine, nitrogen, or methane.
I would do the following.
density (g/L) x 22.4 L/mole = grams/mole which is the molar mass. Then calculate the molar mass of NH3, SO2, Cl2, N2, and CH4 and compare.
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To calculate the molar mass of each substance, we need to use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (which is 1 atm at STP)
V = Volume (which is 1 L at STP)
n = Number of moles
R = Ideal gas constant (0.0821 L·atm/(mol·K))
T = Temperature (which is 273.15 K at STP)
Rearranging the equation, we have:
n = PV/RT
Now, let's calculate the number of moles for each gas using the given densities:
For Gas A:
Density A = 1.25 g/L
Since density is defined as mass/volume, we can rearrange the equation to find the mass:
mass A = density A × volume = 1.25 g/L × 1 L = 1.25 g
Now, we can calculate the number of moles:
n A = mass A / molar mass A
For gases B and C, we perform the same calculations.
For Gas B:
Density B = 2.87 g/L
mass B = density B × volume = 2.87 g/L × 1 L = 2.87 g
n B = mass B / molar mass B
For Gas C:
Density C = 0.714 g/L
mass C = density C × volume = 0.714 g/L × 1 L = 0.714 g
n C = mass C / molar mass C
To calculate the molar mass (M) of each substance, rearrange the equation:
M = mass / n
Now, let's calculate the molar masses:
M A = mass A / n A
M B = mass B / n B
M C = mass C / n C
Once we have calculated the molar masses, we can identify each substance by comparing their molar masses to the molar masses of known substances: ammonia (NH3), sulfur dioxide (SO2), chlorine (Cl2), nitrogen (N2), and methane (CH4).
Compare the calculated molar masses with the molar masses of known substances to identify each gas.