Answer Happy

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2. How did increasing the temperature affect the rate of reaction? Why did this happen? Use lab data to support your answer. 3. Predict what would happen to the rate of reaction at room temperature in the iodine clock reactions in the following scenarios: a If fine crystals of KIO3, rather than a solution, were used. Explain why. b. Compared to your prediction in (a), would the rate be any different if coarse (i.e. large) crystals of KIO3 were added, rather than fine? Explain why. 4. How did the presence of a catalyst affect the rate of reaction for the decomposition of hydrogen peroxide? Why did this happen? Use lab observations to support your answer.
Color Part II. Equilibrium and Le Châtelier's Principle Content Stress Fe(NO3)3 none KSCN none Test tube #1 Fe(NO3)3 & KSCN none add Fe(NO3)3 Test tube #2 Fe(NO3)3 & KSCN Test tube #3 add KSCN Fe(NO3)3 & KSCN Fe(NO3)3 & KSCN Test tube #4 add EDTA Test tube #5 Fe(NO3)3 & KSCN add heat Test tube # 6 Fe(NO3)3 & KSCN remove heat Questions (continued) 5. In which direction (toward reactants or toward products) did the addition of Fe(NO3)3 shift the equilibrium? How do you know? 6. In which direction (toward reactants or toward products) did the addition of KSCN shift the equilibrium? How do you know? 7. In which direction (toward reactants or toward products) did the addition of heat shift the equilibrium? How do you know? 8. In which direction (toward reactants or toward products) did the removal of heat shift the equilibrium? How do you know? 9. Heat can be considered as either a reactant or product, depending upon the reaction involved (i.e., endothermic or exothermic). In this reaction, is heat a reactant or product? How do you know? 10. The ion Fe will react with s? ions to form insoluble (i.e solid) Fe2S3. If a solution of s ions was added to the equilibrium mixture in this study (Fe3+ + SCN = FeSCNP), in which direction would the equilibrium shift and why?