Answer:
The partial pressure of NO2 = 0.152 atm
Explanation:
Step 1: Data given
Pressure NO2 = 0.500 atm
Total pressure at equilibrium = 0.674 atm
Step 2: The balanced equation
2NO2(g) → 2NO(g) + O2(g)
Step 3: The initial pressure
pNO2 = 0.500 atm
pNO = 0 atm
p O2 = 0 atm
Step 4: Calculate pressure at the equilibrium
For 2 moles NO2 we'll have 2 moles NO and 1 mol O2
pNO2 = 0.500 - 2x atm
pNO =2x atm
pO2 = xatm
The total pressure = p(total) = p(NO2) + p(NO) + p(O2)
p(total) = (0.500 - 2x) + 2x + x= 0.674 atm
0.500 + x = 0.674 atm
x = 0.174 atm
This means the partial pressure of NO2 = 0.500 - 2*0.174 = 0.152 atm
4.003 is the mass of helium gas
Answer:
C3H8 + 5O2 ====> 3CO2 + 4H20
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 %
<span>Some
of the solutions exhibit
colligative properties. These properties depend on the amount of solute
dissolved in a solvent. For boiling point elevation, we calculate the increase in temperature by the equation:
</span><span>ΔT(boiling point) =
(Kb)mi
where Kb is a constant, m is the molality of the solution, i is the van't Hoff factor.
From the given data, we can easily calculate for i as follows:
</span>ΔT(boiling point) = (Kb)mi
103.45 - 100 = (0.512)3.90i
i = 1.73 <-------van't Hoff factor
