- (10 pts) The following decomposition reaction of NO2(g)is'2older with rate constant, k 0.255 1./mol•min. 2 NO2(g). 2 NO(g) 02(g) a) Using the differential ratrinssestictn, calculate the initial rate. Rate., of NO2 consumption when (NO21., 0.16M.
b) How many minutes will the reaction need to run before the concentration of remaining [1402], - 0.0404? Mc the integrated 2' order rate law equation here.) - (12 pta) The following data for the reaction NOilaq) N114-(oo)—. 2 Th(g)+ 21i20® is needed to answer the following question& This reaction can be used to ensue nitrogen gat
Expt # Rate. (WO (NO-1 OH MO SO 1 5.40x10-7 0.0100 0.200 2 2.15x10. 0.0400 0.200 3 1.08x10✓ 0.200 0.0200 4 3.20E10 0.200 0.0600
a) What is the general initial rate law equation for this reaction? (lire symbols:. y. and 6) b) Determine the reaction order for each reagent using the data? (rind and y.) c) What is the numerical value of the rate constant. k, with the COMM units? - 112 ptsl Comider the reaction Ht(g) I:(g) 41 2111(g) at 273K. On the LAS. an initial quantity of 0.27M was added of each material to the same container. No RHS material was added initially At equilibrium though. m experiment found that the concentration of the RHS material is (HUN - 0.423. Using this equilibrium information, the ICE scheme with the initial LAS concentrations. and the equilibrium expression, determine the value of K. for this reaction. Stumm 2
- (10 ins) Answer the following questions refemng to the followmg: 014(g) 1120(g) 4-1 3 112(g) CO(g) IC, - 5.5
+C
E
a) If an initial concentration of all four compounds is 2.0111. what is Q..?
b) In which direction will the reaction spontaneouslychange and give a reason? Became all mataul■ at intent mown,. 'on nau comae Kc m Qe m decide 'huh sok mcreate to teach eqmItmum
c)Sa up the ICE scheme directly under the mine° reaction above with the concentration information from part a) and the +1- from pat b). You an not berry asked to why smthing.
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