how is the oxide of arsenic worked out when its in its gas state
please help im flumuxed
Please clarify your question? What do you mean by "worked out?
the question states
determine the molecular formular of the oxide of arsenic when it is in its gaseous state
evidence
arsenic heated at 650c pressure of 890mm hg the 0.927g sample of oxide and vol 194cm3
Use PV = nRT
p is pressure in atmospheres. You have pressure of 890 mm Hg and that is 890/760 = ?? atmospheres.
V is in liters. Your 194 cc = 0.194 L
n = number of mols. Solve for this.
R = constant of 0.08206 L*atm/mol*K
T = 650 C = 273+650 = ?? Kelvin.
Solve for n, THEN
you know mols = grams/molar mass.
You will know mols and grams. solve for molar mass of the oxide.
To determine the molecular formula of the oxide of arsenic in its gaseous state, you can use the ideal gas law equation: PV = nRT.
1. Convert the given pressure from mm Hg to atmospheres: 890 mm Hg / 760 mm Hg/atm = 1.17 atm.
2. Convert the given volume from cm³ to liters: 194 cm³ / 1000 cm³/L = 0.194 L.
3. Rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT.
4. Substitute the given values into the equation:
n = (1.17 atm) * (0.194 L) / [(0.08206 L*atm/mol*K) * (273 K + 650 °C)].
5. Simplify and calculate the value of n.
Next, you can use the molar mass of the sample and the number of moles obtained to determine the molecular formula.
1. Calculate the number of moles using the formula:
moles = grams / molar mass.
2. Substitute the given values into the equation:
moles = 0.927 g / molar mass.
3. Rearrange the equation to solve for the molar mass:
molar mass = grams / moles.
4. Substitute the calculated values from earlier into the equation to determine the molar mass of the oxide.
Finally, the molecular formula of the oxide of arsenic can be determined by comparing the molar mass obtained with the known masses of different compounds and their respective molecular formulas.