I can't actually answer this one if the empirical formula is not given. Luckily, I've found a similar problem from another website. The problem is shown in the picture attached. It shows that the empirical formula is CH₂O. Let's calculate the molar mass of the empirical formula.
Molar mass of E.F = 12 + 2(1) + 16 = 30 g/mol
Then, let's divide this to the molar mass of the molecular formula.
Molar mass of M.F/Molar mass of E.F = 180/30 = 6
Therefore, let's multiply 6 to each subscript in the empirical formula to determine the actual molecular formula.
<em>Actual molecular formula = C₆H₁₂O₆</em>
Explanation:
The given data is as follows.
T = 
= (120 + 273.15)K = 393.15 K,
As it is given that it is an equimolar mixture of n-pentane and isopentane.
So, 
= 0.5 and 
= 0.5
According to the Antoine data, vapor pressure of two components at 393.15 K is as follows.
(393.15 K) = 9.2 bar
(393.15 K) = 10.5 bar
Hence, we will calculate the partial pressure of each component as follows.
= 
= 4.6 bar
and, 
= 
= 5.25 bar
Therefore, the bubble pressure will be as follows.
P = 
= 4.6 bar + 5.25 bar
= 9.85 bar
Now, we will calculate the vapor composition as follows.
= 
= 0.467
and, 
= 
= 0.527
Calculate the dew point as follows.
= 0.5, 
= 0.5
= 0.101966 
P = 9.807
Composition of the liquid phase is 
and its formula is as follows.
= 
= 0.5329
= 
= 0.467
Answer:
The answer to your question is Q = 355.64 J
Explanation:
Data
Heat = Q = ?
Temperature 1 = T1 = 20°C
Temperature 2 = T2 = 37°C
mass = m = 5 g
Specific heat = Cp = 4.184 J/g°C
Formula
Q = mCp(T2 - T1)
-Substitution
Q = (5)(4.184)(37 - 20)
-Simplification
Q = (5)(4.184)(17)
-Result
Q = 355.64 J
Answer:
The elements in__Group_ 0 of the Periodic Table are called the_noble__gases. They are generally __unreactive_. because they have a__full_outer shell of electrons. So they do not need to gain__lose_or share _electrons_ with other atoms.
Answer:
Kb for CH₃NH₂ (methylamine) is 4.4 × 10⁻⁴
Hope that helps.
