A sample of pure NH4HS is placed in a sealed 2.0-L container and heated to 550 K at which the equilibrium constant is 3.5 x 10-3. Once the reaction reaches equilibrium, what mass of NH3 is present in the container

The mass of in the container is 2.074 gram

Explanation:

Given:

Volume of     lit

Equilibrium constant

The reaction in which is produced

  ⇄

Here equal moles of and is formed.

From the formula of equilibrium constant,

      M

Above value shows,

So in 2 L no. moles of = moles.

So mass of 0.122 mole of is = g

Therefore, the mass of in the container is 2.074 gram

beta decay is the answer

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.