1 mole of nitrogen tetraoxide was placed in a container and allowed to dissociate according to the next reaction: N2O4 (g) --> 2NO2 (g)  The resulting mixture occupied a volume of 36 lt at a pressure of 1 atm and at a temperature of 45 C. Calculate: a) The equilibrium constants Kp and Kc. b) If this mixture is heated to 100ºC, the equilibrium pressure is 1.25 atm, determine the equilibrium constant at this temperature

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Ammonia can react with oxygen according to the following two reactions: 4 NH3 + 5 O2  →   4 NO + 6 H2O 2 NH3 + 3/2 O2 →  N2 + 3 H2O 24.7 mole NH3 enter the reactor, along with 171 mole O2.  The reaction proceeds to 0.68 fractional conversion of ammonia and the selectivity of NO over N2 is 4.1.  Determine the mole of oxygen exiting the reactor. Report your answer with two decimal place.

Question 10 The following reaction is first order with a rate constant of 0.529 1/hr: X3Z4 (g) 3X (g) + 4 Z(g) If 3.00 moles of X3Z4 are reacted for 139 minutes, how much (in moles) of Z can be produced? Enter a number to 2 decimal places in moles of Z. 4.91 Question 11 The gas-phase decomposition of NOBR has a k= 0.21 M1 s1 at 10°C. NOBrg → NO(g) + % Br2 (g) rate = k[NOBr]? %D How much of the NO is produced after 1.9 min when the reaction started with 0.08M NOBR? "round your answer up to 4 decimal places