Question

The rising cost and decreasing supply of oil will require alternative fuels for transportation one option currently under research is the use of hydrogen for fuel. Hydrogen can be extracted

From natural gas according to the following reaction:

CH4(g)+CO2(g)--><---2CO(g)+2H2(g)

Kc = 9.819x10^-2 at 825 k

A) an 85.0 l reaction container contains 1259 miles of ch4 and 1259 miles of CO2 at 825K . What mass of h2 in grams is present in the reaction mixture at equilibrium (make sure in terms of molar concentration

B) what is the kp value?

C)now that the reaction has established equilibrium show which direction forward backward of no change it wold have to do to resitablish equilibrium

1) decrease volume of container

2)increase pressure by adding Ar

3) adding additional h2

4)removing some of the CO2

5) adding a catalyst

Answer 1

Answer : Here first thing is to convert the miles into grams and then calculate the molarity [means the concentration of all the terms ]

Now apply Kc = [Product] /[Reactant ] = [CO]² [H2]² /[CH4][CO2] and solve it for the concentration of H2 and then by using molarity equation = moles/volume in L calculate the mass of H2 .

2) In this part we have to use the relation of Kp and Kc which is like

Kp = Kc (RT) ^deln

Here R is the gas constant , T is temperature and deln is the change in number of moles { moles of product - moles of reactant ]

By using it you can calculate the reaquired Kp .

C] 1) by decreasing the volume of container the rate of the reaction increases .

2) Increasing pressure by adding inert gas Ar does not affect the reaction

3) Adding additional H2 hence the concentration of product increases hence the reaction goes in Backward direction.

4) Removing some of CO2 then again the reaction goes backward direction .

5) By adding a catalyst means it increases the rate of reaction but does not affect the reaction .