Answer:
A: 2.525 x 10⁻⁴ mol
B: 2.583 x 10⁻⁴ mol
Explanation:
Part A:
Data Given:
- Temperature of water (H₂O) = 21.3°C
Convert Temperature to Kelvin
T = °C + 273
T = 21.3 + 273 = 294.3 K
- volume of (H₂O) gaseous state = 5.1 mL
Convert mL to liter
1000 mL = 1 L
5.1 ml = 5.1/1000 = 0.0051 L
Solution
no. of moles can be calculated by using ideal gas formula
PV = nRT
Rearrange the equation for no. of moles
n= PV / RT . . . . . . . . . (1)
where
P = pressure
V = Volume
T= Temperature
n = Number of moles
R = ideal gas constant
where
R = 0.08206 L.atm / mol. K
Now put the value in formula (1) to calculate no. of moles of
n = 1.2 atm x 0.0051 L / 0.08206 L.atm.mol⁻¹. K⁻¹ x 294.3 K
n = 0.0061 atm.L / 24.162 L.atm.mol⁻¹
n = 2.525 x 10⁻⁴ mol
no. of moles of gas (H₂O) = 2.525 x 10⁻⁴ mol
_______________
Part B:
Data Given:
- Temperature of water (H₂) = 21.3°C
Convert Temperature to Kelvin
T = °C + 273
T = 21.3 + 273 = 294.3 K
- volume of (H₂) gas = 5.2 mL
Convert mL to liter
1000 mL = 1 L
5.2 ml = 5.2/1000 = 0.0052 L
Solution
no. of moles can be calculated by using ideal gas formula
PV = nRT
Rearrange the equation for no. of moles
n= PV / RT . . . . . . . . . (1)
where
P = pressure
V = Volume
T= Temperature
n = Number of moles
R = ideal gas constant
where
R = 0.08206 L.atm / mol. K
Now put the value in formula (1) to calculate no. of moles of
n = 1.2 atm x 0.0052 L / 0.08206 L.atm.mol⁻¹. K⁻¹ x 294.3 K
n = 0.0062 atm.L / 24.162 L.atm.mol⁻¹
n = 2.583 x 10⁻⁴ mol
no. of moles of gas (H₂) = 2.583 x 10⁻⁴ mol
