From your notation, it is phosphorus trichloride. Basically, there are three molecules of phosphorus chloride.
Answer:
3.1atm
Explanation:
Given parameters:
Volume of gas = 2L
Number of moles = 0.25mol
Temperature = 25°C = 25 + 273 = 298K
Unknown:
Pressure of the gas = ?
Solution:
To solve this problem, we use the ideal gas equation.
This is given as;
PV = nRT
P is the pressure
V is the volume
n is the number of moles
R is the gas constant = 0.082atmdm³mol⁻¹K⁻¹
T is the temperature
P =
Now insert the parameters and solve;
P =
= 3.1atm
Answer:
"
" is the right answer.
Explanation:
Given:
Partial pressure of
,
= 0.20 atm
Partial pressure of
,
= 0.15 atm
at ![400^{\circ} C](https://tex.z-dn.net/?f=400%5E%7B%5Ccirc%7D%20C)
As we know,
⇒ ![K_p = \frac{pN_2\times pH_2^3}{pNH_3^2}](https://tex.z-dn.net/?f=K_p%20%3D%20%5Cfrac%7BpN_2%5Ctimes%20pH_2%5E3%7D%7BpNH_3%5E2%7D)
By putting the values, we get
![1.5\times 10^3=\frac{0.20\times (0.15)^3}{pNH_3^2}](https://tex.z-dn.net/?f=1.5%5Ctimes%2010%5E3%3D%5Cfrac%7B0.20%5Ctimes%20%280.15%29%5E3%7D%7BpNH_3%5E2%7D)
![pNH_3^2 = \frac{0.000675}{1.5\times 10^3}](https://tex.z-dn.net/?f=pNH_3%5E2%20%3D%20%5Cfrac%7B0.000675%7D%7B1.5%5Ctimes%2010%5E3%7D)
![=6.7\times 10^{-4} \ atm](https://tex.z-dn.net/?f=%3D6.7%5Ctimes%2010%5E%7B-4%7D%20%5C%20atm)
Answer:
The answer is D if it's wrong let me know pls