Answer:
168.72 grams
Explanation:
Density = Mass/Volume
Volume = 14.8
Mass = ?
Density = 11.4
Let x = mass
11.4 = x/14.8
Multiply both sides by 14.8
14.8(11.4 = x/14.8)
x = 168.72
I have a feeling that #2 is the one.
Answer:
The value of equilibrium constant is 29.45.
Explanation:
Moles of hydrogen gas = 2.00 mol
Concentration of hydrogen gas =![[H_2]= \frac{2.00 mol}{1.00 L}=2.00 M](https://tex.z-dn.net/?f=%5BH_2%5D%3D%20%5Cfrac%7B2.00%20mol%7D%7B1.00%20L%7D%3D2.00%20M)
Moles of iodine gas = 1.00 mol
Concentration of iodine gas =![[I_2]= \frac{I.00 mol}{1.00 L}=1.00 M](https://tex.z-dn.net/?f=%5BI_2%5D%3D%20%5Cfrac%7BI.00%20mol%7D%7B1.00%20L%7D%3D1.00%20M)
![H2(g) + I2(g)\rightleftharpoons 2 HI(g)](https://tex.z-dn.net/?f=H2%28g%29%20%2B%20I2%28g%29%5Crightleftharpoons%202%20HI%28g%29)
initially
2.00 M 1.00 M 1.00 M
At equilibrium:
(2.00-x/2) (1.00-x/2) x
Moles of HI at equilibrium = 1.80 M
Concentration of HI at equilibrium =![[HI]=\frac{1.80 mol}{1.00L} = 1.80M= x](https://tex.z-dn.net/?f=%5BHI%5D%3D%5Cfrac%7B1.80%20mol%7D%7B1.00L%7D%20%3D%201.80M%3D%20x)
The expression of an equilibrium constant is given by ;
![K_c=\frac{[HI]^2}{[H_2][I_2]}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BHI%5D%5E2%7D%7B%5BH_2%5D%5BI_2%5D%7D)
![K_c=\frac{x^2}{(2.00-\frac{x}{2})(1.00-\frac{x}{2})}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7Bx%5E2%7D%7B%282.00-%5Cfrac%7Bx%7D%7B2%7D%29%281.00-%5Cfrac%7Bx%7D%7B2%7D%29%7D)
Putting x equal to 1.80 M.
![K_c=\frac{(1.80)^2}{(2.00-\frac{1.80}{2})(1.00-\frac{1.80}{2})}=29.45](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%281.80%29%5E2%7D%7B%282.00-%5Cfrac%7B1.80%7D%7B2%7D%29%281.00-%5Cfrac%7B1.80%7D%7B2%7D%29%7D%3D29.45)
The value of equilibrium constant is 29.45.