I think the half of 1293 its the mass ? maybe idk I just tried
<u>Answer:</u> The equilibrium constant for the given equation is 0.0315
<u>Explanation:</u>
We are given:
Total pressure in the container = 0.596 atm
The given chemical equation follows:
![N_2H_6CO_2(s)\rightleftharpoons 2NH_3(g)+CO_2(g)](https://tex.z-dn.net/?f=N_2H_6CO_2%28s%29%5Crightleftharpoons%202NH_3%28g%29%2BCO_2%28g%29)
<u>Initial:</u> -
<u>At eqllm:</u> - 2x x
Evaluating the value of 'x'
![\Rightarrow (x+2x)=0.596\\\\x=0.199](https://tex.z-dn.net/?f=%5CRightarrow%20%28x%2B2x%29%3D0.596%5C%5C%5C%5Cx%3D0.199)
The expression of
for above equation follows:
![K_p=p_{CO_2}\times (p_{NH_3})^2](https://tex.z-dn.net/?f=K_p%3Dp_%7BCO_2%7D%5Ctimes%20%28p_%7BNH_3%7D%29%5E2)
The partial pressure of pure solids and pure liquids are taken as 1 in the equilibrium constant expression.
Putting values in above expression, we get:
![K_p=(0.199)\times (2\times 0.199)^2\\\\K_p=0.0315](https://tex.z-dn.net/?f=K_p%3D%280.199%29%5Ctimes%20%282%5Ctimes%200.199%29%5E2%5C%5C%5C%5CK_p%3D0.0315)
Hence, the equilibrium constant for the given equation is 0.0315
The density of a sample of nitrogen gas (N₂) that exerts a pressure of 5.30 atm in a 3.50-L container at 125°C is 4.54 gm/litre
<h3>What is the
Ideal Gas Law ?</h3>
This law combines the relationships between p, V, T and mass, and gives a number to the constant.
The ideal gas law is:
pV = nRT
where n is the number of moles, and R is universal gas constant.
The value of R depends on the units involved, but is usually stated with S.I. units as: R = 8.314 J/mol·K
The values given in the question are
p= 5.30 atm , V=3.50 L
T (in Kelvin) = 125+273 K
= 398 K
R = 0.0821 L·atm /mol·K
The Ideal Gas equation can be re written as
pM=DRT
M is the molar mass , D is the density
M for N₂ is 28 gm/mol
so density can be determined as
![\rm D= \dfrac{p M}{RT} \\\\\rm D= \dfrac{5.3\; \times 28}{0.082 \;\times398} \\\\\rm D =4.54 gm/litres](https://tex.z-dn.net/?f=%5Crm%20D%3D%20%5Cdfrac%7Bp%20M%7D%7BRT%7D%20%5C%5C%5C%5C%5Crm%20D%3D%20%5Cdfrac%7B5.3%5C%3B%20%5Ctimes%2028%7D%7B0.082%20%5C%3B%5Ctimes398%7D%20%5C%5C%5C%5C%5Crm%20D%20%3D4.54%20gm%2Flitres)
Therefore the density of a sample of nitrogen gas (N₂) that exerts a pressure of 5.30 atm in a 3.50-L container at 125°C is 4.54 gm/litre
To know more about Ideal Gas Law
brainly.com/question/13821925
#SPJ1
Energy cannot be created or destroyed, so the answer would be c.) not a or b.
Hope this helps!