The equilibrium constant for the reaction:

2no(g)+br2(g) < -> 2nobr(g) is kc= 1.3x10^-2 at 1000 k.

1. at this temperature does the equilibrium favor no and br2, or does it favor nobr?
2. calculate kc for 2nobr(g) < -> 2no(g)+br2(g)
3. calculate kc for nobr(g) < -> no(g)+1/2 br2(g)

1. NO and Br₂

2. 77

3. 8.8

Explanation:

Let's consider the following reaction.

2 NO(g) + Br₂(g) ⇄ 2 NOBr(g)

The equilibrium constant for this reaction is:

1. At this temperature does the equilibrium favor NO and Br₂, or does it favor NOBr?

Since Kc₁ < 1, the reactants are favored, that is, NO and Br₂.

2. Calculate Kc for 2 NOBr(g) ⇄ 2 NO(g) + Br₂(g)

The equilibrium constant is:

3. Calculate Kc for NOBr(g) ⇄ NO(g) + 1/2 Br₂(g)

The equilibrium constant is:

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.