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6. Consider the equation: 2NO2(g) → N2(g) +202() What effect will the following changes have on the reaction rate (...
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following...
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following changes would cause less NH3 to be produced? decreasing the volume adding N2 increasing the volume adding H2 2. Consider the following reaction. N2(g) + 3 H2(g) ⇋ 2 NH3(g) The forward reaction is exothermic. Which of the following changes would cause less NH3 to be produced? decreasing the temperature adding H2 increasing the temperature adding N2 3. What is the effect of a...
1- Identify the changes in the following system at equilibrium when the temperature is suddenly decreased....
1- Identify the changes in the following system at
equilibrium when the temperature is suddenly decreased. The
reaction is endothermic. PCl5 <> PCl3+Cl2
2- A reaction profile (not to scale!) for the reaction
O2+NO2=O3+NO
3- A reaction profile (not to scale!) for the reaction
C2H5Br+H-=C2H5OH+Br-
l the Relerences to access important values if needed for this question. Identify the changes in the following system at equilibrium when the temperature is suddenly decreased The reaction is endothermic. The value of K...
27. Consider the following chemical reaction: N2(g) + 2O2(g) ----> 2NO2(g) decreasing the pressure of reaction...
27. Consider the following chemical reaction: N2(g) + 2O2(g) ----> 2NO2(g) decreasing the pressure of reaction mixture will decrease amounts of O2(g) have no effect on the reaction increase amounts of N2(g) increase amounts of NO2(g) 26. Consider the following chemical reaction: CO(g) + Cl2(8) ----------> COCl2(g) At the beginning 0.400 M CO(g) is mixed with 0.0500 M C12(8). At equilibrium, 0.0100 M of the product is produced. Calculate the equilibrium constant. K-0.641 K - 1.99x 10exp-3 K-8.81 OK -...
Consider the following reaction that has reached equilibrium: (3 pts) 13. AH-52.2 kJ N2 (g) +...
Consider the following reaction that has reached equilibrium: (3 pts) 13. AH-52.2 kJ N2 (g) + 202 (g)今2NO2 (g) What will happen to the concentration of O2 if the temperature is raised? a. b. What will happen to the concentration of NO2 if the pressure is raised? What will happen to the concentration of N2 if the pressure is lowered? c.
29 (6 pts) How do concentration of reactants, temperature and catalysts affect the rate of a chemical reaction? Exp...
29 (6 pts) How do concentration of reactants, temperature and catalysts affect the rate of a chemical reaction? Explain. Concentration of reactants: mcreases more collisions within the reactants. collisions Temperature: Increase in temperature causes increase in more and more energy in collisions. (increases rate? Catalyst: Lowens energy of activation of reactants cate? (increases rutes
Given the following reactions Question 1 Given the following reactions AH 66.4 k N2 (g)+202 (g)2NO2...
Given the following reactions
Question 1 Given the following reactions AH 66.4 k N2 (g)+202 (g)2NO2 (g) 2NO (g)+02 (g) 2NO2 (g) AH=-114.2 k the enthalpy of the reaction of the nitrogen to produce nitric oxide 2NO (g) N2 (g)+02 (g) KJ. is 90.3 180.6 -180.6 47.8 47.8
The rate law for the reaction 2 NO2 (g) + F2 (g) → 2 NO2F (g)...
The rate law for the reaction 2 NO2 (g) + F2 (g) → 2 NO2F (g) is rate = K[NO2][F2]. Which of the following will lead to a change in the rate constant, k? The pressure of NO2 is decreased by 1/2 OA: k changeslo B: k does not change The volume of the container is doubled IOA: k changes o B: k does not change The temperature of the reaction is decreased O A: k changesloB: k does not...
What changes will result in a loss of color for the following reaction? N2O4(g) -> 2NO2(g)...
What changes will result in a loss of color for the following reaction? N2O4(g) -> 2NO2(g) dH < 0 <- colorless brown I. Increasing temperature II. Decreasing volume III. Addition of No2.
1) Determine the effect of each of the following changes on the equilibrium mixture for the...
1) Determine the effect of each of the following changes on the equilibrium mixture for the following reaction: N2(g) + O2(g) + 90.2 kJ + 2NO(g) Circle an answer for each change. a. Increasing the temperature Shift to reactants No change Shift to products b. Adding a catalyst Shift to reactants No change Shift to products c. Removing nitrogen monoxide gas Shift to reactants No change Shift to products d. Decreasing the volume of the container Shift to reactants No...
1. What is AG at 25 °C (298 K) for the reaction below? Show your answer...
1. What is AG at 25 °C (298 K) for the reaction below? Show your answer with four significant figures Cs) + 026) CO268 AH=-393.5 kJ/mol AS=0.0029 kJ/mol K 2. A certain reaction has AH = 10.3 kJ/mol and AS = 42.7J/K-mol. Calculate AG in kJ/mol at 338 K. Show your answer with four significant figures 3. Consider the following potential energy diagram that represents two different reactions. Which reaction is spontaneous? Which reaction is faster? Reaction A Reaction B...
1- Identify the changes in the following system at
equilibrium when the temperature is suddenly decreased. The
reaction is endothermic. PCl5 <> PCl3+Cl2
2- A reaction profile (not to scale!) for the reaction
O2+NO2=O3+NO
3- A reaction profile (not to scale!) for the reaction
C2H5Br+H-=C2H5OH+Br-
l the Relerences to access important values if needed for this question. Identify the changes in the following system at equilibrium when the temperature is suddenly decreased The reaction is endothermic. The value of K...
27. Consider the following chemical reaction: N2(g) + 2O2(g) ----> 2NO2(g) decreasing the pressure of reaction mixture will decrease amounts of O2(g) have no effect on the reaction increase amounts of N2(g) increase amounts of NO2(g) 26. Consider the following chemical reaction: CO(g) + Cl2(8) ----------> COCl2(g) At the beginning 0.400 M CO(g) is mixed with 0.0500 M C12(8). At equilibrium, 0.0100 M of the product is produced. Calculate the equilibrium constant. K-0.641 K - 1.99x 10exp-3 K-8.81 OK -...
Consider the following reaction that has reached equilibrium: (3 pts) 13. AH-52.2 kJ N2 (g) + 202 (g)今2NO2 (g) What will happen to the concentration of O2 if the temperature is raised? a. b. What will happen to the concentration of NO2 if the pressure is raised? What will happen to the concentration of N2 if the pressure is lowered? c.
29 (6 pts) How do concentration of reactants, temperature and catalysts affect the rate of a chemical reaction? Explain. Concentration of reactants: mcreases more collisions within the reactants. collisions Temperature: Increase in temperature causes increase in more and more energy in collisions. (increases rate? Catalyst: Lowens energy of activation of reactants cate? (increases rutes
Given the following reactions
Question 1 Given the following reactions AH 66.4 k N2 (g)+202 (g)2NO2 (g) 2NO (g)+02 (g) 2NO2 (g) AH=-114.2 k the enthalpy of the reaction of the nitrogen to produce nitric oxide 2NO (g) N2 (g)+02 (g) KJ. is 90.3 180.6 -180.6 47.8 47.8
The rate law for the reaction 2 NO2 (g) + F2 (g) → 2 NO2F (g) is rate = K[NO2][F2]. Which of the following will lead to a change in the rate constant, k? The pressure of NO2 is decreased by 1/2 OA: k changeslo B: k does not change The volume of the container is doubled IOA: k changes o B: k does not change The temperature of the reaction is decreased O A: k changesloB: k does not...
1) Determine the effect of each of the following changes on the equilibrium mixture for the following reaction: N2(g) + O2(g) + 90.2 kJ + 2NO(g) Circle an answer for each change. a. Increasing the temperature Shift to reactants No change Shift to products b. Adding a catalyst Shift to reactants No change Shift to products c. Removing nitrogen monoxide gas Shift to reactants No change Shift to products d. Decreasing the volume of the container Shift to reactants No...
1. What is AG at 25 °C (298 K) for the reaction below? Show your answer with four significant figures Cs) + 026) CO268 AH=-393.5 kJ/mol AS=0.0029 kJ/mol K 2. A certain reaction has AH = 10.3 kJ/mol and AS = 42.7J/K-mol. Calculate AG in kJ/mol at 338 K. Show your answer with four significant figures 3. Consider the following potential energy diagram that represents two different reactions. Which reaction is spontaneous? Which reaction is faster? Reaction A Reaction B...
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