1. A dust explosion occurs in a saw mill. a catalytic converter. Cataluct Concentratin 8. Calcium carbonate (CaCO3) deteriorates as a result of its reaction with the pollutant sulfur dioxide. The 9. The reaction between zinc and hydrochloric acid occurs within seconds if the zinc metal is finely powdered. 10. Food can spoil quickly when left on the kitchen counter. However, a refrigerator slows that process so that the same food remains fresh for days. onlentration sunfoce area Temperatme SCIENCE 10 - Q4 W8: Applications of Factors Affecting Rate of Chemical Reactions Direction: Applying the concepts of factors affecting chemical reaction, analyze whether the given situations increase or decrease the rate of the given reaction, then explain your answer on the table below. C6H1206 + 6 O2 > 6 H20+ 6 CO2 Does this increase or decrease the rate of reaction? Change in Condition Explain why kample: 1. Increasing the temperature 2. Increasing the concentration of CH12O, 3. Decreasing the concentration of O2 4. Increase the surface area by chewing up food in your mouth 5. Decreasing the temperature 6. Increasing the pressure in the container 7. Decreasing the concentration of H20 B. Increasing the volume of the container where the reaction occurs in - Increasing the concentration of CO2 D. Using a catalyst (like salivary amylase)

When the sign of an energy change is being determined, this would always be with respect to what?

Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.

Calculate AGO at 605 K for H₂O(g) + 1/2 02(g) → H₂O₂(g) using the following data: AGO = H₂(g) +O₂(g) → H₂O₂(g) K = 8.9 × 10³6 at 605 K 2H₂(g) + O₂(g) → 2H₂O(g) K = 2.0 x 106 at 605 K kJ/mol

18. The thermochemical equation for the formation of ammonia from nitrogen and hydrogen is as follows: N2(g) + 3H2 (g) 5 2NH3 (g) AH=-92,2 kJ Given the system is initially at equilibrium, which of the following actions would cause the reaction to shift to the left? a. removing NH3 (g) b. removing H2 (g) c. decreasing the temperature d. adding a catalyst e. adding N2 (g)

What is the effect of equilibrium when heat is removed (cooled) from the system? CO + H2O ⟷ CO2 + H2 ΔH = +41.4 kJ Group of answer choices Neither reactant nor products would be produced. Shift left. Both reactants and products would be produced. Shift right. This equation does not represent an equilibrium system.

Ammonia (NH3) decomposes to form nitrogen gas and hydrogen gas with an enthalpy of 89.4kJ/mol. Aclosed container is charged with 6.0 atm ammonia and heated to 25.0°C. At equilibrium the pressure of H2 is3.60atm. a. Write the balanced reaction.