<u>Answer:</u> The partial pressure of gas number 3 is 159 mmHg
<u>Explanation:</u>
Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.
To calculate the partial pressure of gas number 3, we use the law given by Dalton, which is:

We are given:
Total pressure of the tank,
= 950 mmHg
Vapor pressure of gas number 1,
= 335 mmHg
Vapor pressure of gas number 2,
= 456 mmHg
Putting values in above equation, we get:
![950=335+456+p_3\\\\p_{3}=[950-(335+456)]=159mmHg](https://tex.z-dn.net/?f=950%3D335%2B456%2Bp_3%5C%5C%5C%5Cp_%7B3%7D%3D%5B950-%28335%2B456%29%5D%3D159mmHg)
Hence, the partial pressure of gas number 3 is 159 mmHg
Answer:
the answer is 74.03%
Explanation:
Add all the masses together, M of C = 120.1, M of H = 14.4 and M of N = 28.02. Adding all those together will give you the mass of the compound, then u divide the mass of carbon by the mass of compound and multiply by 100 to get the percent by mass.
120.1 + 14.4 + 28.02 = 162.26
120.1/162.26 x 100 = 74.03%
Answer:
pCH4 = 0.9184 atm
pCCl4 = 0.9184 atm
pCH2Cl2 = 0.2832 atm
Explanation:
Step 1: Data given
The equilibrium constant, Kp= 9.52 * 10^-2
Temperature = 350 K
Each have an initial pressure of 1.06 atm
Step 2: The balanced equation
CH4(g) + CCl4(g) ⇆ 2CH2Cl2(g)
Step 3: The pressure at the equilibrium
pCH4 = 1.06 - X atm
pCCl4 = 1.06 - X atm
pCH2Cl2 = 2X
Step 4: Calculate Kp
Kp = (2X)² / (1.06 - X)*(1.06 - X)
9.52 * 10^-2 = 4X² / (1.06 - X)*(1.06 - X)
X = 0.1416
Step 5: Calculate the partial pressure
pCH4 = 1.06 - 0.1416 = 0.9184 atm
pCCl4 = 1.06 - 0.1416 = 0.9184 atm
pCH2Cl2 = 2 * 0.1416 = 0.2832 atm
Kp = (0.2832²) / (0.9184*0.9184)
Kp = 9.52 * 10^-2
pCH4 = 0.9184 atm
pCCl4 = 0.9184 atm
pCH2Cl2 = 0.2832 atm
Answer:
Diastereomers can have different physical properties and reactivity. They have different melting points and boiling points and different densities.