The answer is 0.975 L

Volume = mol/Molarity

We have molarity (0.788 M) and we need mol and volume. Let's first calculate number of moles of CaCl2 in 85.3 g:

Molar mass of CaCl2 is sum of atomic masses of Ca and Cl:
Mr(CaCl2) = Ar(Ca) + 2Ar(Cl) = 40 + 2 * 35.45 = 40 + 70.9 = 110.9 g/mol

So, if 110.9 g are in 1 mol, 85.3 g will be in x mol:
110.9 g : 1 mole = 85.3 g : x
x = 85.3 g * 1 mole / 110.9
x = 0.769 moles

Now, calculate the volume:
V = 0.769/0.788
V = 0.975 L

5 0

3 years ago

Determine the volume occupied by 0.352 mole of a gas at 25⁰C if the pressure is 81.8 kPa.

lions [1.4K]

Data:
p (pressure) = 81.8 kPa = 81.8*10³ Pa ≈ 8.07 atm
v (volume) = ? (in L)
n (number of mols) = 0.352 mol
R (Gas constant) = 0.082 (atm*L/mol*K)
T (temperature) = 25ºC converting to Kelvin, we have:
TK = TC + 273 → TK = 25 + 273 → TK = 298

Formula:
$p*V =n*R*T$

Solving:
$p*V =n*R*T$
$8.07*V = 0.352*0.082*298$
$8.07V \approx 8.60$
$V \approx \frac{8.60}{8.07}$
$\boxed{\boxed{V \approx 1.06\:L}}$

7 0

3 years ago