Can anyone help me with these two questions: At a certain temperature, the equil

Question

Can anyone help me with these two questions:

At a certain temperature, the equilibrium constant for the following chemical equation is 2.00. SO_2(g) + NO_2(g) SO_3(g) + NO(g) At this temperature, calculate the number of moles of NO_2(g) that must be added to 2.86 mol of SO_2(g) in order to form 1.30 mol of SO_3(g) at equilibrium. At a certain temperature, the equilibrium constant, K_c, for this reaction is 53.3. H_2(g) + I_2(g) 2HI(g) K_c = 53.3 At this temperature. 0.700 mol of H_2 and 0.700 mol of l_2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?

Explanation / Answer

1) SO2 + NO2 <-------> SO3 + NO K = 2 so K = [SO3][NO]/ [ SO2][NO2]

we have 2.86mol of SO2 and want make 1.30mol of SO3 for this we need know how many NO2 mol need so

K = [SO3][NO]/ [ SO2][NO2] =) [NO2] = [SO3][NO]/ [ SO2]K as [SO3] = [NO]

[NO2]  = [SO3][NO]/ [ SO2]K =  [NO2]  = [SO3]2/ [ SO2]K replacing for your value we have

[NO2]  = [SO3]2/ [ SO2]K =  [NO2]  = [1.3]2/( [ 2.86] x 2 ) = 0.30mol of  [NO2]

2) H2 + I2 <--------> 2HI Kc = 53.3 so  Kc = [HI]2/ [H2][I2 ]

Kc = [HI]2/ [H2][I2 ] =)  Kc = [HI] = (Kc[H2][I2 ] )1/2 replacin for your value

Kc = [HI] = (Kc[H2][I2 ] )1/2 =  Kc = [HI] = (53.3 x 0.7M x 0.7M )1/2 = 5.11M

[HI] = 5.11M

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