Answer:
50 degrees C I am going to assume
0 degrees C is 273.15 K so 50 plus 273.15 is 323.15K
Explanation:
You would have to use the ideal gas law: PV = nRT where,
P = pressure
V = volume
n = moles
R = universal gas constant for a specific pressure (in this case it's 62.364 torr)
T = temperature in Kelvin
First, convert Celsius to kelvin by adding 273 to 25, which gives you 298K
Now plug in your variables to find n:
(800 torr)(1.25 L) = n(62.364)(298K)
1000 = 18584.472n
Now divide 1000 by 18584.472 to get n:
1000/18584.472 = 0.054 moles
The equilibrium constant expression for this reaction that takes place in water and involve ions can be written as K= [H_3 O^+ ][OH^- ]/([H_2 O] ^2 ). But the concentration of undissociated water, H_2 O is much larger than the concentration of the ions that is essentially remains constant. Therefore, we can include it in the equilibrium constant. The resulting new equilibrium constant can be written: K_W= [H_3 O^+ ][OH^- ].
3.) likely to form an ionic bond
Metals and non-metals combine to form ionic bonds.
