Answer:
Explanation:
<u>1. Calculate the iniital concentration of HI(g) introduced</u>
The initial concentration of HI(g), [HI(g)], is the number of moles per liter:
- [HI(g)] = 0.316mol/1liter = 0.316M
<u>2. Build the ICE (initial, change, equilibrium) table</u>
ICE table:
2HI(g) → H₂(g) + I₂(g)
I 0.316 0 0
C - 2x +x +x
E 0.316 - 2x x x (x = 3.12×10⁻²M)
<u>3. Find the equilibrium constant, Kc</u>
Answer:
Yes, there will be liquid present and the mass is 5.19 g
Explanation:
In order to do this, we need to use the equation of an ideal gas which is:
<em>PV = nRT (1)</em>
<em>Where:</em>
<em>P: Pressure</em>
<em>V: Volume</em>
<em>n: number of moles</em>
<em>R: gas constant</em>
<em>T: Temperature</em>
we know that the pressure is 856 Torr at 300 K. So, if we want to know if there'll be any liquid present, we need to calculate the moles and mass of the CCl3F at this pressure and temperature, and then, compare it to the initial mass of 11.5 g.
From (1), solving for moles we have:
<em>n = PV/RT (2)</em>
Solving for n:
P = 856/760 = 1.13 atm
R = 0.082 L atm / mol K
n = 1.13 * 1 / 0.082 * 300
n = 0.0459 moles
Now, the mass is:
m = n * MM (3)
The molar mass of CCl3F reported is 137.37 g/mol so:
m = 0.0459 * 137.37
m = 6.31 g
Finally, this means that if we put 11.5 g of CCl3F in a container, only 6.31 g will become gaseous, so, this means it will be liquid present, and the mass is:
m = 11.5 - 6.31
m = 5.19 g
I'm pretty sure its momentum
Answer:
- All alkalies are bases but all bases are not alkalies
- all alkalies are soluble in water but all bases are not alkalies .
hope it is helpful to you