Question

a. Classify each of the following chemical reactions as a combination, decomposition, single-replacement, double-replacement, or combustion reaction. Justify your answers. 2KNO3 â†’ 2KNO2 + O2 b. Zn + 2AgNO3 â†’ Zn(NO3)2 + 2Ag c. Ni(NO3)2 + 2NaOH â†’ Ni(OH)2 + 2NaNO3 2. Assign an oxidation number to each atom of the following compounds or polyatomic ions. a. P2O5 b. KMnO4 c. NO3- 3. By using oxidation numbers, determine whether the following reaction is a redox reaction or a nonredox reaction. Justify your answer. 4NH3 + 3O2 â†’ 2N2 + 6H2O 4. For the redox reaction below: Identify the following and provide an explanation for each answer. a. The substance oxidized. b. The substance reduced. c. The oxidizing agent. 5. Write the equilibrium constant expression for each of the following reactions. Justify your answers. 6. Calculate the value of the equilibrium constant, K, for the equilibrium system 2NO(g) â†”ï¸ N2(g) + O2(g) at 1000Â°C, given that the equilibrium concentrations are 0.0026 M for NO, 0.024 M for N2, and 0.024 M for O2. 7. How will the gas-phase equilibrium below CH4(g) + 2H2S(g) + heat â†”ï¸ CS2(g) + 4H2(g) Shift by each of the following? a. The removal of H2(g) b. The addition of CS2(g) c. An increase in the temperature 8. Predict the shift in equilibrium position that will occur for each of the following processes when the volume is reduced: a. The preparation of liquid phosphorus trichloride b. The reaction of phosphorus trichloride with ammonia

          a. Classify each of the following chemical reactions as a combination, decomposition, single-replacement, double-replacement, or combustion reaction. Justify your answers. 
2KNO3 â†’ 2KNO2 + O2 
b. Zn + 2AgNO3 â†’ Zn(NO3)2 + 2Ag 
c. Ni(NO3)2 + 2NaOH â†’ Ni(OH)2 + 2NaNO3 

2. Assign an oxidation number to each atom of the following compounds or polyatomic ions. 
a. P2O5 
b. KMnO4 
c. NO3- 

3. By using oxidation numbers, determine whether the following reaction is a redox reaction or a nonredox reaction. Justify your answer. 
4NH3 + 3O2 â†’ 2N2 + 6H2O 

4. For the redox reaction below: Identify the following and provide an explanation for each answer. 
a. The substance oxidized. 
b. The substance reduced. 
c. The oxidizing agent. 

5. Write the equilibrium constant expression for each of the following reactions. Justify your answers. 

6. Calculate the value of the equilibrium constant, K, for the equilibrium system 2NO(g) â†”ï¸ N2(g) + O2(g) at 1000Â°C, given that the equilibrium concentrations are 0.0026 M for NO, 0.024 M for N2, and 0.024 M for O2. 

7. How will the gas-phase equilibrium below CH4(g) + 2H2S(g) + heat â†”ï¸ CS2(g) + 4H2(g) Shift by each of the following? 
a. The removal of H2(g) 
b. The addition of CS2(g) 
c. An increase in the temperature 

8. Predict the shift in equilibrium position that will occur for each of the following processes when the volume is reduced: 
a. The preparation of liquid phosphorus trichloride 
b. The reaction of phosphorus trichloride with ammonia

Added by Steven B.

Question

Please give Ace some feedback