The molar solubility of Ag2CO3 is 0.074M at 10°C.
What is the Ksp of Ag2CO3 at the same degree?

0.00162 is the Ksp of Ag2CO3 at 10 degrees.

Explanation:

Ag2CO3(s) --- 2Ag+ (aq) + CO3 ^-2(aq)

The product of molar solubility of each ion in moles/litre gives the solubility product.

The molar solubility of Ag2CO3 is 0.074 M at 10 degrees.

From the above reaction we can see that

2 Moles of Ag and 1 mole of carbonate ions,

So,  [Ag2CO3]= 2[Ag]^2[CO3^2-]

Ksp of Ag+= 2*0.074  

= 0.148

Ksp of CO3^-2=  0.074

    = 0.148

Ksp of AgNO3= [0.148]^2 [0.074]

Ksp of AgNO3  = 0.00162 AT 10 degrees

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.