Consider The Equilibrium Reaction 2no G O2 G 2 No2 G Ah 27 Kj Mol Of No2 G Increasing The Temperature Of The 1 (33.7 KiB) Viewed 41 times
Consider the equilibrium reaction: 2NO(g) + O2(g) 2 NO2 (g) AH = -27 kJ/mol of NO2(g) Increasing the temperature of the system at constant pressure will cause: (a) an increase in the concentration of NO2(g) (b) a decrease in the volume of the system (c) an increase in the concentration of O2(g) (d) a decrease in the concentration of NO (9) O O a b C d
Analysis of the equilibrium: 2NOCI 2NO(g) + Cl2(g) gave the following concentrations [NOCI] = 0.50 mol/L, [NO] = 2.0x10-² mol/L, and [Cl₂] = 1.0x10-² mol/L. What is the value of Kc for this equilibrium? 4.0x10-4 (b) (a) (d) (c) 1.3x10-5 8.0x10-6 1.6x10-5 1.3x105 (e) d. [H3PO4] [H₂PO4 ][H*] e. [H3PO4] / [PO4³-][H+1³ a b d e Question 8 (1 point) For phosphoric acid, H3PO4, the Ka₁ = a. [PO4³-][H+1³/[H3PO4] b. [HPO42-][H]/[H3PO4] C. [H₂PO4][H] / [H3PO4] (₁) a b d e (D
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