Ideal solutions obey Raoult's law, which states that:
P_i = x_i*(P_pure)_i
where
P_i is the partial pressure of component i above a solution
x_i is the mole fraction of component i in the solution
(P_pure)_i is the vapor pressure of pure component i
In this case,
P_benzene = 0.59 * 745 torr = 439.6 torr
P_toluene = (1-0.59) * 290 torr = 118.9 torr
The total vapor pressure above the solution is the sum of the vapor pressures of the individual components:
P_total = (439.6 + 118.9) torr = 558.5 torr
Assuming the gas phase also behaves ideally, the partial pressure of each gas in the vapor phase is proportional to its molar concentration, so the mole fraction of toluene in the vapor phase is:
118.9 torr/558.5 torr = 0.213
Lunch of a patient has 3 oz skinless chicken, 3 oz of broccoli, 1 medium apple, and 1 cup of nonfat milk
Energy content of 3 oz skinless chicken is = 110 kcal
Energy content of 3 oz broccoli = 30 kcal
Energy content of 1 medium apple = 60 kcal
Energy content of 1 cup non-fat milk = 90 kcal
So the kilocalories of energy patient obtained from lunch
= 110 kcal+ 30 kcal + 60 kcal + 90 kcal = 290 kcal
Acid more H3O+ than OH-
Base less H3O+ than OH-
Answer:
% yield = 58.33 %
Explanation:
∴ moles X = 2.00 mol
∴ moles Y = 2.00 mol
∴ moles Z = 1.75 mol = moles produced
- % Yield = ( moles produced / theoretical moles ) × 100
theoretical moles:
⇒ moles Z = (2.00 mol X)*(3 mol Z/2 mol X) = 3.00 mol Z
⇒ % yield = [(1.75 mol produced)/(3.00 theoretical mol)]×100
⇒ % yield = 58.33 %
