Consider the following reaction: 6 NiO(s) + 4 CCF_3(g) rightarrow 6 NiF_2(s) + 2

Question

Consider the following reaction: 6 NiO(s) + 4 CCF_3(g) rightarrow 6 NiF_2(s) + 2 Cl_2(g) + 3 O_2(g) A researcher combines a 0.60 mol of NiO with exactly 0.40 mol of ClF_3(g) in a sealed flask and waits until the reaction goes to completion If the total pressure at the start of the reaction was 0.25 atm, what will be the total pressure in the flask at the end of the reaction? 0.060 atm 0.31 atm 0.55 atm 0.69 atm Given the following information at 298 K: SnO_2 (s) + 2 H_2(g) Sn(s) + 2 H_2O(g) K_1 = 8.12 H_2(g) +CO_2 (g) H_2O (g) + CO(g) K_2 = 0.771 Determine the K for the overall reaction SnO_2(s) + 2 CO(g) Sn(g) + 2 CO_2 (g). 13.7 7.12 6.58

Explanation / Answer

(2) From the balanced equation provided,

4 mol of gaseous reactants produce 5 moles of gaseous products

yhen ,

0.4 mol of gaseous reactans produces 0.5 mol of gaseous products.

and

it is given that pressure exerted by 0.4 mol gas = 0.25 atm

then pressure exerted by 0.5 mol of gas = 0.5 * 0.25 / 0.4 = 0.3125 atm

SO, the answer is (b)

(3) We get final equation by doing

(1) - 2*(2)

So, Equilibrium constant of final equation, K = K1 / 2K2 = 8.12 / (2*0.771) = 5.26

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