University:
High School
Course:
High School Chemistry
Academic year:

2023
Views:

290

Pages:

2
Author:

Sheha A.

Name:_________________________ per:___ Worksheet- Reaction Rates Use this reaction for the questions below: C6H12O6 (s) + 6 O2(g)  6 H2O (g) + 6 CO2 (g) 1. What happens to the concentrations of: a. C6H12O6 & O2 as the reaction proceeds ? b. H2O + CO2 as the reaction proceeds ? 2. According to the collision theory, what 3 circumstances are needed for C6H12O6 & O2 to react? 3. What is the activation energy for a chemical reaction? 4. Use the equation & the collision theory to explain: C6H12O6 (s) + 6 O2(g)  6 H2O (g) + 6 CO2 (g) Change in condition: a. Increasing the temperature Does this increase or decrease the rate of reaction? Ex: Increases (speeds up) Explain why Ex: Molecules move faster & collide more = Increased rxn rate b. Increasing the concentration of C6H12O6 c. Decreasing the concentration of O2 d. Increase the surface area by chewing up food in your mouth e. Decreasing the temperature f. Increasing the pressure in the container g. Decreasing the concentration of H2O h. Increasing the volume of the container the reaction occurs in Increasing the concentration of CO2 i. j. Using a catalyst (like salivary amylase) 5. On the accompanying energy diagram, label the following terms: a. reactants b. products c. activation energy 6. On the graph to the right, draw and label what this diagram would look like if a catalyst was added to the reaction. 7. Graph reading a. How much energy (#) do the reactants have? b. How much energy (#) do the products have? c. How much energy (#) is required to activate this un-catalyzed reaction? d. Is this reaction endothermic or exothermic? How do you know? Equilibrium & Le Chatelier’s Principle 1. What 2 characteristics define a system at equilibrium? 2. What 3 factors are considered to be stresses on an equilibrium system? 3. According to Le Chatelier, how does a system at equilibrium respond to a stress? 4. Complete the chart below: Products of  (forward) reaction Reaction a. CH4 + O2 <--> CO2 + H2O + heat Products of  (reverse) reaction Is the  (forward) reaction endothermic/ exothermic? (890.3 kJ) b. NaCl (s) + heat <--> Na+ + Clc. H2O(l) + heat <--> H2O(g) Using Le Chatelier’s principle, predict how each of the changes would affect the equilibrium systems Ex: Shifts to right (towards products), shifts to left (towards reactants), or No change occurs 5. N2(g) + 3 H2(g) <--> 2 NH3(g) + 92 kJ a. Stress: Adding extra H2 Relief: use excess H2 a. Stress: Adding CO How: Shifts  Relief: b. Stress: Extra NH3 (ammonia) is added Relief: 6. CH3OH (l) + 18 kJ <--> CO (g) + 2 H2 (g) How: b. Stress: Removing heat How: Relief: How: c. Stress: Adding extra N2 c. Stress: Removing CH3OH Relief: Relief: How: d. Stress: Removing H2 Relief: How: d. Stress: Decrease the volume of the container How: Relief: e. Stress: The pressure is increased e. Stress: Relief: Relief: How: How: Adding Heating How: f. Stress: Increase the volume of the container f. Stress: Decreasing the pressure Relief: Relief: How: How: g. Stress: Heating the system g. Stress: Removing H2 Relief: Relief: How: How: 7. C2H4 (g) + H2 (g) <--> C2H6 (g) + heat What stresses would force the reaction to shift  (to the right)? a) Pressure (increase/decrease): b) Temperature: c) Concentrations (of C2H6, C2H4, H2)