Initially at 300 K and 10 atm pressure, 1 mol of a gas is allowed to expand adiabaticall against a constant pressure of 4 atm until equilibrium is achieved. Assume the gas to b with Cp,m = 28.58 + 1.76 x 10-2 T

For the following reaction: A(g) + 3 B(g) magnitude of Kp (don't report the units) assuming the following composition at equilibrium: PA = 0.735 bar PB = 0.603 bar Pc = 0.627 bar PD 0.87 bar = 2 C(g) + D(g) Calculate the =

As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C

What is Boyle's law constant, kp if a sealed rigid container with a volume, Vof 0.600 L has a pressure, Pof 130.0 kPa? V = kg(1/P) BIUA - A - I E E E X x, = E 12pt Paragraph fx MacBook Air

The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if Kc and Qc are within 5% of each other.) (a.) 2 SO3(g)  2 SO2(g) + O2(g) Pi(SO3) = 0.100 atm, Pi(SO2) = 1.10 atm, Pi(O2) = 1.20 atm, Kp = 5.5 atm   What is the reaction quotient?   What direction will the reaction shift to?        LEFT or RIGHT?   (b.) 2 NO(g) + Cl2(g)  2 NOCl(g) Pi(NO) = 1.25 atm, Pi(Cl2) = 1.25 atm, Pi(NOCl) = 0 atm,  Kp = 3.1 ✕ 103   What is the reaction quotient?   What direction will the reaction shift to?        LEFT or RIGHT?   (c.) N2(g) + O2(g)  2 NO(g) [N2]i = 0.120 M, [O2]i = 0.240 M, [NO]i = 1.20 M,  Kc = 0.050   What is the reaction quotient?   What direction will the reaction shift to?        LEFT or RIGHT?

Consider the following reaction where K, = 9.52×10-2 at 350 K: %3D CH4(g) + CC14(g) 2CH2C1½(g) If the three gases are mixed in a rigid container at 350 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: • 1. A reaction will occur in which CH,Cl2(g) is consumed. v 2. K, will increase. • 3. A reaction will occur in which CH, is consumed. • 4. Q is less than K. v 5. The reaction is at equilibrium. No further reaction will occur.

Consider the equilibrium system described by the chemical reactionbelow. Calculate the value of Qc for the initial set reaction conditions in3.00 L container:8.65 g C2H4, 11.2 g O2, and 5.68 g CH3CHO. 2 C2H4(g) + O2(g) = 2 CH3CHO(g)

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Determine the equilibrium partial pressure of NH3 in a reaction vessel that initially contained 0.900 atm N2 and 0.500 atm H2 at 648 K.

Calculate the pressure equilibrium constant KP for the equilibrium between nitrogen monoxide, oxygen, and nitrogen dioxide has the final temperature of the mixture round your answer to two significant digits.