The mass in a chemical reaction remains (mostly) the same.
(except for radiation/nuclear fission, in which mass gets converted into energy)
Cm^3 = mL
1.11 g/cm^3 = 1.11 g/mL
Density (g/mL) multiplied by volume (mL) will give us the mass (g)
1.11 g/mL * 385 mL = 427.35 g
And since we have 3 significant figures, we have 427. g.
Answer:
2.06 × 10⁻¹⁰
Explanation:
Let's consider the solution of a generic compound AB₂.
AB₂(s) ⇄ A²⁺(aq) + 2B⁻(aq)
We can relate the molar solubility (S) with the solubility product constant (Kps) using an ICE chart.
AB₂(s) ⇄ A²⁺(aq) + 2B⁻(aq)
I 0 0
C +S +2S
E S 2S
The solubility product constant is:
Kps = [A²⁺] × [B⁻]² = S × (2S)² = 4 × S³ = 4 × (3.72 × 10⁻⁴)³ = 2.06 × 10⁻¹⁰
We first assume that the gas is an ideal gas so we can use the relation PV= nRT where P is the pressure, V is the volume, n is the number of moles R is the gas constant and T is the temperature. In a closed system, the number of moles should be constant since mass cannot be created or destroyed. So the only thing we can manipulate here is the volume of the system. We do as follows:
PV/T = nR = k
P1V1/T1 = P2V2/T2
V2 = P1V1T2/T1P2
V2 = 1.50 (298.15) V1 / (273.15)(1.0)
V2 = 1.64V1
Therefore, the volume should be changed by a factor of 1.64 of the original volume.
