i just need help on the last two pictures! not the first one . thank you

Ammon will decompose into nitrogen and hydrogen at high temperature, an industrial chemist studying this reaction files a 200 ml. Bank with 1,7 m of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 1.0 am Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your miswer to 2 sgrifiche agits. X A chemical engineer is studying the following reaction HCH, CO,(aq)+ CHNH (aq) CH, CO,(aq)+CH, NH(aq) At the temperature the engineer picks, the equilibrium constant for this reaction is 0.54 The engineer charges (ills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below Predict the changes in the compositions the engineer should expect next time she measures the compositions reaction vessel concentration expected change in concentration 0.50 M Increase Older the change 021 M increas Older (change) 0.85M compound HCH.CO CH, NH , CH,NE , CHNH increase o decrease Che change) 100 M increase I decrease (no change 135M increase I decrease 60 Charge 0.97M increase @ . decrease (no danga 1.00 M o increase I decrease (no change) 135 M of increase I decrease (no change) 0.97 M Increase I decrease (no change 0.12 M t increase O decrease (no change) CH,NH HCH,CO, CH, NH, CH,CO CH, NH , CH, NE, CH,CO. CH,NH 0.24M of increase decrease (no change 133 M increase I decrease (no change) OSIM Increase O decrease (no change 0.69 M o increase O decrease (no change 0.85 M Increase decrease (no change X X 5