What is the solution's freezing point: 15 g of CH4N2O (Molar mass = 60.055 g/mol) in 200. g of H2O? (Kf = 1.86 (°C·kg)/mol)
1 answer:
Ok to answer this question we firsst need to fin the number of mol of Urea (CH4N2O). to do this we simply :
1 mol of urea =15/60.055 = 0.25mol
therefore 200g of water contain 0.25mol
the next step is to determine the malality of our solution in 200g of water, to do this we say:
200 g = 1Kg/1000g = 0.2kg
therefor 0.25mol/0.2Kg = 1.25mol/kg
and from the equation:
we know that i = 1
we are given Kf
b is the molality that we just calculated
therefore;
the solutions freezing point is -2.325°C
You might be interested in
Answer:
<h2>6.91 </h2>Explanation:
To find the pH we must first find the pOH
The pOH can be found by using the formula
pOH = - log [ {OH}^{-} ]
We have
pOH = 7.09
Next we use the equation
pH = 14 - pOH
We have
pH = 14 - 7.09
We have the final answer as
<h3>6.91</h3>Hope this helps you
11.48-gram of are needed to produce 6.75 Liters of
gas measured at 1.3 atm pressure and 298 K
The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).
First, calculate the moles of the gas using the gas law,
PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.
Given data:
P= 1.3 atm
V= 6.75 Liters
n=?
R=
T=298 K
Putting value in the given equation:
Moles = 0.3588 moles
Now,
Mass= 11.48 gram
Hence, 11.48-gram of are needed to produce 6.75 Liters of
gas measured at 1.3 atm pressure and 298 K
Learn more about the ideal gas here:
#SPJ1