Answer:
Solubility of O₂(g) in 4L water = 3.42 x 10⁻² grams O₂(g)
Explanation:
Graham's Law => Solubility(S) ∝ Applied Pressure(P) => S =k·P
Given P = 0.209Atm & k = 1.28 x 10⁻³mol/L·Atm
=> S = k·P = (1.28 x 10⁻³ mole/L·Atm)0.209Atm = 2.68 x 10⁻³ mol O₂/L water.
∴Solubility of O₂(g) in 4L water at 0.209Atm = (2.68 x 10⁻³mole O₂(g)/L)(4L)(32 g O₂(g)/mol O₂(g)) = <u>3.45 x 10⁻² grams O₂(g) in 4L water. </u>
Answer:
As temperature increases the volume of given amount of gas increases while pressure and number of moles remain constant.
Explanation:
According to the charle's law,
The volume of given amount of gas is directly proportional to the temperature at constant pressure and number of moles of gas.
Mathematical expression:
V ∝ T
V = KT
V/T = K
When temperature changes from T₁ to T₂ and volume changes from V₁ to V₂.
V₁/T₁ = K V₂/T₂ = K
or
V₁/T₁ = V₂/T₂
Thus, the ratio of volume and temperature remain constant for constant amount of gas at constant pressure.
Answer:
6 inches and that should be the answer
The answer is C by vibrating the molecules in the matter
Answer:
1109 g H₂O
Explanation:
2.2 pounds can be converted to grams using a conversion ratio:
(2.2lb)(453.592g/lb) = 997.9024 g C₅₇H₁₁₀O₆
The mass in grams is converted to moles using the molecular weight of tristearin (891.48 g/mol)
(997.9024 g)(mol/891.48g) = 1.119...mol C₅₇H₁₁₀O₆
The moles of C₅₇H₁₁₀O₆ can be related to the moles of water through the molar ratio:
(1.119mol C₅₇H₁₁₀O₆)(110 H₂O/2 C₅₇H₁₁₀O₆) = 61.545 mol H₂O
The mass of water is then calculated using the molecular weight (18.02 g/mol):
(61.545 mol)(18.02 g/mol) = 1109 g H₂O
