Question

[References Use the References to access important values if needed for this question Consider the following reaction where Ke - 1.20x10 at 500 K: PCI; (B) = PCI(g) + Cl (8) A reaction mixture was found to contain 0.135 moles of PCIS (R). 4.81x102 moles of PCI (R), and 4.19x10 moles of Ch (R), in a 1.00 liter cont Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium PCI(g) must be consumed. 2. In order to reach equilibrium Ke must decrease 3. In order to reach equilibrium PC1z must be produced 4. Qc is greater than K 5. The reaction is at equilibrium. No further reaction will occur. Submit Answer Retry Entire Group more group attempts remaining

Answer 1

Pels Pc +cl. 0.135 moles È 4.81x10² moles + 4.19x10² moes 0.0481 moles 0.0419 moles, Equilibrium constant ake = 1.20x10² - 2 n=cu 0.135 Here, Qc = [[cly] [che] [pcls 6:487) -(0:0481)(0.0919) Concentration no. of moes Volume = 0.01499 = 1:49 x162 Q 1.49x10² is greater than the actual ke value. A. and kc are concentration products devided by concentration of reactants. But ac is at any conteni time. Kc is at equilibrium. Here Qe >kc, there are more products than reactants. To reach equilibrium the reaction will produce more produits. reactants. 1) false (Pols should be produced through back. - ward reaction. 2) False C should decrease than kc). 3) False (pte pelz should not be produced. 4) True (Qc > Kc). 5) false (Reaction is not at equibrium. At eatm