14.41 For the reaction H2(g) + CO2(g) = H,0(g) + CO(g) at 700°C, Ke moles of H2 that are present at equilibrium if a mix- ture of 0.300 mole of CO and 0.300 mole of H,O is heated to 700°C in a 10.0-L container. 0.534. Calculate the number of acksp. A4 10 00 V NO gas decomposes:

For the reaction: 2 IBr(g) qe I2(g) + Br2(g), Kc = 3.57 * 10-3 (150 ̊C), held within a 1.00 L flask  If 0.500 M I2 and 0.500 M Br2 are allowed to reach equilibrium, what are the equilibrium concentrations of I2, Br2 and IBr?

3. Please don't write on a paper. I can't understand handwritten.

8:02 Question 4 of 8 Submit Consider the equilibrium system described by the chemical reaction below. The decomposition of NOBR has a value Kc equal to 3.07 x 10-4 at 297 K. If an initial solution of 0.20 M NOBR decomposes, what will the concentration of NO be at equilibrium? 2 NOBr(g) = 2 NO(g) + Br2(g) 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. 2 NOBR(g) = 2 NO(g) Br2(g) + Initial (M) Change (M) Equilibrium (M) 5 RESET 0.20 0.40 +x +x2 +2x +2x? -x -2x -2x² 0.20 - x 0.20 + x 0.40 - x 0.40 + x 0.20 - 2x 0.20 + 2x 0.40 - 2x 0.40 + 2x Tap here or pull up for additional resources

Consider the following equilibrium: CO (g) + Br2 (g) = COBr2 (g) K=12.0 at 85C Initially, the concentration of CO is 0.10M and Br2 is 0.40M. What are all the equilibrium concentrations?

3) What would happen to the position of the equilibrium when the following changes are made to the reaction below? Hgo (3) + Hg ) + O2 (9) (a) Hgo is added to the system. (b) The pressure on the system increases.