1. Convert Units
* Volume (V): 825 mL = 0.825 L (since 1 L = 1000 mL)
* Temperature (T): 25 °C = 298.15 K (since K = °C + 273.15)
* Pressure (P): 7.90 x 10^2 torr = 1.04 atm (since 1 atm = 760 torr)
2. Ideal Gas Law Equation
The Ideal Gas Law is: PV = nRT
Where:
* P = Pressure (in atm)
* V = Volume (in L)
* n = Number of moles
* R = Ideal gas constant (0.0821 L·atm/mol·K)
* T = Temperature (in K)
3. Solve for n (number of moles)
Rearrange the equation to solve for n:
n = PV / RT
4. Plug in the Values
n = (1.04 atm) * (0.825 L) / (0.0821 L·atm/mol·K) * (298.15 K)
5. Calculate
n ≈ 0.035 moles
Answer: The chemistry student collected approximately 0.035 moles of gas.
