At a particular temperature, a 3.0-L flask contains 2.4 mol Clh, 1.0 mol NOCI, a

Question

At a particular temperature, a 3.0-L flask contains 2.4 mol Clh, 1.0 mol NOCI, and 4.5 x 103 mol NO. Calculate K at this temperature for the following reaction: 1. 2NOCI(g)2NO)+Chg) At a particular temperature, 8.0 mol NO2 is placed into a 1.0-L container and the NO2 dissociates by the reaction: 2. 2N02(g)--NO(g) + O2(g) At equilibrium the concentration of NO(g) is 2.0 M. Calculate K for this reaction. 3. Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction equilibrium constants (Kp values) as a function of temperature are 300°C. 4.34×10 : 500°C. 145×105 600°C, 2.25× 106 Is the reaction exothenmic or endothermic?

Explanation / Answer

Hi i am sorry to say that as per chegg guidelines experts can answer only one full question (1st question only). Hence i request you to please post remaining question as seperate. Thanks in advance for understanding the situation.

2NOCl <==> 2NO + Cl2

NOCl concentration = 1.0 mol / 3 liter = 0.034 M

Cl2 concentration = 2.4 mol / 3 liter = 0.8 M

NO concentration = 0.0045 mol / 3 liter = 0.0015 M

K = [(NO)2(Cl2)] / [NOCl]2 = [(0.0015 M)2(0.8 M)] / [0.034 M]2 = 0.00155709342

K = 1.56 x 10-3 -------------------------------Equilibrium constant

Since they have given concentrations only, so we have to calculate Kc instead of Kp.

Hope this helped you!

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