What is the molar mass of a compound given that 0.035g of the gaseous compound occupies 30cm3 at r.t.p
To find the molar mass of a compound, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (atmospheres)
V = volume (liters)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (Kelvin)
At r.t.p. (room temperature and pressure), the temperature is 273.15 Kelvin and the pressure is 1 atmosphere.
We are given:
Mass = 0.035g
Volume = 30cm^3 (which is 0.03L)
First, we need to convert the mass from grams to moles using the molar mass formula:
Molar mass = mass / moles
Let's assume that the molar mass is M grams/mol. Then we can solve for moles:
moles = mass / M
We know that 1 mole of any gas at r.t.p. occupies 22.4 L, so we can rewrite the ideal gas law equation as:
P * V = n * R * T
1 * 0.03 = (mass / M) * 0.0821 * 273.15
Now, we can rearrange the equation to solve for M:
M = (mass * R * T) / (P * V)
Substituting the given values:
M = (0.035 * 0.0821 * 273.15) / (1 * 0.03)
M = 5.459 g/mol
Therefore, the molar mass of the compound is approximately 5.459 g/mol.
To determine the molar mass of the compound, we need to use the ideal gas law equation.
The ideal gas law equation is:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles
R is the ideal gas constant
T is the temperature
At r.t.p (standard temperature and pressure), the values are:
P = 1 atm (atmospheric pressure)
V = 30 cm3 (volume)
T = 273 K (temperature)
First, convert the volume from cm3 to liters (L):
30 cm3 = 30/1000 L = 0.03 L
Rearranging the ideal gas law equation, we can solve for n (the number of moles):
n = PV / RT
Now we can substitute the values into the equation:
n = (1 atm) * (0.03 L) / (0.0821 atm L/mol K * 273 K)
Next, we calculate the number of moles:
n = 0.00104 mol
Lastly, we can calculate the molar mass by dividing the mass of the compound (0.035 g) by the number of moles (0.00104 mol):
molar mass = 0.035 g / 0.00104 mol
Therefore, the molar mass of the compound is approximately 33.65 g/mol.
To find the molar mass of a compound, you need to know the mass of the compound and the number of moles present. In this case, you are given the mass of the compound, which is 0.035 grams.
To calculate the number of moles, you can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
At standard temperature and pressure (STP), the pressure is 1 atmosphere (atm) and the temperature is 273.15 Kelvin (K). The volume given is 30 cm3, but it needs to be converted to liters (L) for the equation to work. So, 30 cm3 is equal to 0.030 liters.
Now we can solve for the number of moles (n). Rearranging the equation, we have n = PV / RT.
Plugging in the known values:
P = 1 atm
V = 0.030 L
R = 0.0821 L·atm/(mol·K)
T = 273.15 K
n = (1 atm)(0.030 L) / (0.0821 L·atm/(mol·K))(273.15 K)
n = 0.00118 mol (rounded to four decimal places)
Now that you know the number of moles of the compound, you can calculate the molar mass. The molar mass is the mass of one mole of a substance. In this case, it is the mass of 0.00118 moles of the compound.
Molar mass = mass / number of moles
Molar mass = 0.035 grams / 0.00118 moles
Calculating this value, the molar mass is approximately 29.66 grams/mol (rounded to two decimal places).