Answer:
a. Molarity= ![M =2.1x10^{-1}M](https://tex.z-dn.net/?f=M%20%3D2.1x10%5E%7B-1%7DM)
b. Molality= ![m=2.0x10^{-1}m](https://tex.z-dn.net/?f=m%3D2.0x10%5E%7B-1%7Dm)
Explanation:
Hello,
In this case, given the information about the aniline, whose molar mass is 93g/mol, one could assume the volume of the solution is just 200 mL (0.200 L) as no volume change is observed when mixing, therefore, the molarity results:
![M=\frac{n_{solute}}{V_{solution}} =\frac{3.9g*\frac{1mol}{93g} }{0.2L} =2.1x10^{-1}M](https://tex.z-dn.net/?f=M%3D%5Cfrac%7Bn_%7Bsolute%7D%7D%7BV_%7Bsolution%7D%7D%20%3D%5Cfrac%7B3.9g%2A%5Cfrac%7B1mol%7D%7B93g%7D%20%7D%7B0.2L%7D%20%3D2.1x10%5E%7B-1%7DM)
Moreover, the molality:
![m=\frac{n_{solute}}{m_{solvent}} =\frac{3.9g*\frac{1mol}{93g} }{0.2L*\frac{1.05kg}{1L} } =2.0x10^{-1}m](https://tex.z-dn.net/?f=m%3D%5Cfrac%7Bn_%7Bsolute%7D%7D%7Bm_%7Bsolvent%7D%7D%20%3D%5Cfrac%7B3.9g%2A%5Cfrac%7B1mol%7D%7B93g%7D%20%7D%7B0.2L%2A%5Cfrac%7B1.05kg%7D%7B1L%7D%20%7D%20%3D2.0x10%5E%7B-1%7Dm)
Best regards.
Answer:
The correct answer is - 2770000 cm.
Explanation:
1 kilometer = 1000 meter
1 meter = 100 centimeter
1 kilometer = 100*1000 cm
1 km = 100000 cm.
then,
27.7 kilometers = 2.77 × 10^6 centimeters
So, 27.7 kilometers = 27.7 × 100000
= 2.77 × 106 or 2770000 centimeters.
Answer:
The total pressure is 27.8 atm
Explanation:
From the ideal gas equation,
PV = nRT
P (total pressure) = nRT/V
n (total moles of gases) = (6/1 moles of hydrogen) + (15.2/14 moles of nitrogen) + (16.8/4 moles of helium) = 6+1.1+4.2 = 11.3 moles
R = 0.082057L.atm/gmol.K, T = 27°C = 27+273K = 300K, V = 10L
P = 11.3×0.082057×300/10 = 27.8 atm
Answer:- 0.800 moles of the gas were collected.
Solution:- Volume, temperature and pressure is given for the gas and asks to calculate the moles of the gas.
It is an ideal gas law based problem. Ideal gas law equation is used to solve this. The equation is:
PV=nRT
Since it asks to calculate the moles that is n, so let's rearrange this for n:
![n=\frac{PV}{RT}](https://tex.z-dn.net/?f=n%3D%5Cfrac%7BPV%7D%7BRT%7D)
V = 19.4 L
T = 17 + 273 = 290 K
P = 746 mmHg
we need to convert the pressure from mmHg to atm and for this we divide by 760 since, 1 atm = 760 mmHg
![P=746mmHg(\frac{1atm}{760mmHg})](https://tex.z-dn.net/?f=P%3D746mmHg%28%5Cfrac%7B1atm%7D%7B760mmHg%7D%29)
P = 0.982 atm
R = ![0.0821\frac{atm.L}{mol.K}](https://tex.z-dn.net/?f=0.0821%5Cfrac%7Batm.L%7D%7Bmol.K%7D)
Let's plug in the values in the equation to get the moles.
![n=\frac{0.982atm*19.4L}{0.0821\frac{atm.L}{mol.K}*290K}](https://tex.z-dn.net/?f=n%3D%5Cfrac%7B0.982atm%2A19.4L%7D%7B0.0821%5Cfrac%7Batm.L%7D%7Bmol.K%7D%2A290K%7D)
n = 0.800 moles
So, 0.800 moles of the gas were collected.