Answer:
option (d) is false.
Explanation:
Acid dissociation equilibrium of HCN is represented as-
Acid dissociation constant, 
, is represented as-
![K_{a}=\frac{[H^{+}][CN^{-}]}{[HCN]}](https://tex.z-dn.net/?f=K_%7Ba%7D%3D%5Cfrac%7B%5BH%5E%7B%2B%7D%5D%5BCN%5E%7B-%7D%5D%7D%7B%5BHCN%5D%7D)
where species inside third bracket represents equilibrium concentrations of respective species
So, evidently, presence of excess 
(or NaCN) in solution will combine with 
to produce HCN. Hence will be larger that it would be if only the HCN solution were present.
According to Le-chatlier principle, addition of HCN will shift equilibrium towards right and addition of NaCN will shift equilibrium towards left to keep constant value at a particular temperature.
NaOH gives acid-base reaction with HCN to produce NaCN and water. So, addition of NaOH will increase concentration of and decrease concentration of HCN
Answer:
The soup gets so hot it releases a gas state and it gets trapped in the lid. So the gas gets transformed into a gas into a liquid temperarily.
Explanation:
Answer:
I think u mean molar mass of ca(Mno4)2
if so it is 277.949 g/ mol
<span>Lithium chloride is LiCl (because the valence of lithium is +1 and the valence of chlorine is -1). So the chemical equation is: Li Cl(s) ----> Li(s) + Cl2 (g). To balance the equation you need to multilply both Li Cl (s) and Li(s) by two, and then you finally get the balanced equation: 2 LiCl ---> 2 Li(s) + Cl2(g). Note that the number 2 to the right of Cl is a subscript.</span>
