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Consider the following reaction mechanism: step 1: 2 NO_2 rightarrow NO + NO_3 step 2: NO_3...
A proposed mechanism for the reaction of NO_2 and CO is 2 NO_2(g) rightarrow NO(g) +...
A proposed mechanism for the reaction of NO_2 and CO is 2 NO_2(g) rightarrow NO(g) + NO_3(g) (Slow, endothermic) NO_3(g) + CO(g) rightarrow NO_2(g) + CO_2(g) (Fast, exothermic) a) Write the overall reaction. b) Identify each of the following as a reactant, product, , or intermediate, NO_2, CO, NO_3, CO_2, NO. c) Draw a reaction coordinate for this reaction. Indicate on this drawing the activation energy for each step and the overall enthalpy change. d) Give a plausible rate law.
Consider the following chemical reaction, at 500degree C and 200atm, for question 1-5: Step1: NO_2(g) +...
Consider the following chemical reaction, at 500degree C and 200atm, for question 1-5: Step1: NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) Step 2: NO_2(g) + F_2(g) rightarrow NO_2F(g) rate determining step After this two-step process occurs, what is the overall balanced chemical equation? NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) NO_2(g) + F_2(g) rightarrow NO_2F(g) + F_2(g) 2NO_2(g) + F_2(g) rightarrow 2NO_2F(g) 2NO_2(g) + F_(g) rightarrow 4NO_(g) + F(g) What is the intermediate this multistep mechanism? NO_2(g) F_(g) NO_2F_(g) F_2(g)...
Which of the following reactions is a Redox reaction? Cu(s) + 4HNO_3 rightarrow Cu(NO_3)_3 + 2...
Which of the following reactions is a Redox reaction? Cu(s) + 4HNO_3 rightarrow Cu(NO_3)_3 + 2 NO_2 + 2H_2O Cu(NO_3)_3 + 2 NaOH rightarrow Cu(OH)_2 + 2NaNO_3 Cu(OH)_2 + HCI rightarrow CuCl_2 + H_2O (a) (I) (b) (II) (c) (III) (d) All of them
The decomposition of ozone is the stratosphere can occur by the following two-step mechanism: Br +...
The decomposition of ozone is the stratosphere can occur by the following two-step mechanism: Br + O_3 rightarrow BrO + O rightarrow Br + O_2 which species is an intermediate in this mechanism? A. Br B. BrO C. O D. O_3 Calculate K_c for the reaction 2 Hl (g) - H_2 (g) - H_2 (g) + I_2 (g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L. [I_2] = 0.27 mol/L. A. 5.25...
The following reaction was allowed to come to equilibrium at 35 degree C. The initial molar...
The following reaction was allowed to come to equilibrium at 35 degree C. The initial molar concentration for SO_3 is 0.675 M ([SO_3| = 0.675 M) and the initial molar concentration for CO_2 is 0.444 M (|CO_2] = 0.444 M). After the reaction reached equilibrium the concentration of CO_2 now equals 0.214 M ((CO_2] = 0.214 M). What is the K_c value for the reaction? 0.00987 0.0342 7.31 11.8 16.7 At 35 degree C the equilibrium constant value (K_c) for...
Consider the following reaction where K_c = 77.5 at 600 K. CO(g) + Cl_2(g) COCl_2(g) A...
Consider the following reaction where K_c = 77.5 at 600 K. CO(g) + Cl_2(g) COCl_2(g) A reaction mixture was found to contain 2.42 times 10^-2 moles of CO(g), 4.19 times 10^-2 moles of Cl_2(g) and 0.121 moles of COCl_2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q_c, equals The reaction must run in the forward direction to reach equilibrium. must run in...
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at...
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at 298 K. Delta G degree (NO_2(g)) = 51.84 kJ/mol, Delta G degree (N_2 O_4 (g)) = 98.28 kJ/mol. Calculate Delta G at 298 K if the partial pressures of NO_2 and N_2O_4 are 0.37 atm and 1.62 atm, respectively. Express your answer using one significant figure.
Consider the following reaction between carbon monoxide and hydrogen, CO(g) + 2 H_2(g) Equilibrium CH_3OH(l) K_p...
Consider the following reaction between carbon monoxide and hydrogen, CO(g) + 2 H_2(g) Equilibrium CH_3OH(l) K_p = 2.25 times 10^4 Give the K_p expression for this reaction Determine the equilibrium pressure of CO if the P(H_2) at equilibrium = 0.52 atm If the Q_p for a particular reaction mixture was measure as 2.30 times 10^-4, how will this reaction proceed?
The following reaction is performed at a certain temperature and these data are acquired. Please use...
The following reaction is performed at a certain temperature and these data are acquired. Please use the reaction and data to answer the NEXT 2 QUESTIONS: NO_2 (g) + H_2 O_2 (aq) NO_3 (g) + H_2 O (g); Delta H = -16.15 KJ/mol; K_c = 144 If a scientist observes this reaction at the same temperature starting with 4 M of NO_2 and 4 M of H_2 O_2, what will be the final concentration of NO_3? A. 0.7 M B....
Suppose a reaction occurs with the following mechanism: Step 1: 2AD Step 2: D+E- (fast) B+C...
Suppose a reaction occurs with the following mechanism: Step 1: 2AD Step 2: D+E- (fast) B+C (slow) 1. What is the overall reaction? [Select] 2. What is the intermediate in the mechanism? (Select] 3. What is the molecularity of step 1? (Select 4. Which step is the rate determining step? [Select) 5. What is the rate law predicted by this mechanism? [Select) Question 22 15 pts Consider the following reaction at equilibrium: CO(g) + 2H2(g) CH2OH(g) AH=-18 kJ How will...
A proposed mechanism for the reaction of NO_2 and CO is 2 NO_2(g) rightarrow NO(g) + NO_3(g) (Slow, endothermic) NO_3(g) + CO(g) rightarrow NO_2(g) + CO_2(g) (Fast, exothermic) a) Write the overall reaction. b) Identify each of the following as a reactant, product, , or intermediate, NO_2, CO, NO_3, CO_2, NO. c) Draw a reaction coordinate for this reaction. Indicate on this drawing the activation energy for each step and the overall enthalpy change. d) Give a plausible rate law.
Consider the following chemical reaction, at 500degree C and 200atm, for question 1-5: Step1: NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) Step 2: NO_2(g) + F_2(g) rightarrow NO_2F(g) rate determining step After this two-step process occurs, what is the overall balanced chemical equation? NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) NO_2(g) + F_2(g) rightarrow NO_2F(g) + F_2(g) 2NO_2(g) + F_2(g) rightarrow 2NO_2F(g) 2NO_2(g) + F_(g) rightarrow 4NO_(g) + F(g) What is the intermediate this multistep mechanism? NO_2(g) F_(g) NO_2F_(g) F_2(g)...
Which of the following reactions is a Redox reaction? Cu(s) + 4HNO_3 rightarrow Cu(NO_3)_3 + 2 NO_2 + 2H_2O Cu(NO_3)_3 + 2 NaOH rightarrow Cu(OH)_2 + 2NaNO_3 Cu(OH)_2 + HCI rightarrow CuCl_2 + H_2O (a) (I) (b) (II) (c) (III) (d) All of them
The decomposition of ozone is the stratosphere can occur by the following two-step mechanism: Br + O_3 rightarrow BrO + O rightarrow Br + O_2 which species is an intermediate in this mechanism? A. Br B. BrO C. O D. O_3 Calculate K_c for the reaction 2 Hl (g) - H_2 (g) - H_2 (g) + I_2 (g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L. [I_2] = 0.27 mol/L. A. 5.25...
The following reaction was allowed to come to equilibrium at 35 degree C. The initial molar concentration for SO_3 is 0.675 M ([SO_3| = 0.675 M) and the initial molar concentration for CO_2 is 0.444 M (|CO_2] = 0.444 M). After the reaction reached equilibrium the concentration of CO_2 now equals 0.214 M ((CO_2] = 0.214 M). What is the K_c value for the reaction? 0.00987 0.0342 7.31 11.8 16.7 At 35 degree C the equilibrium constant value (K_c) for...
Consider the following reaction where K_c = 77.5 at 600 K. CO(g) + Cl_2(g) COCl_2(g) A reaction mixture was found to contain 2.42 times 10^-2 moles of CO(g), 4.19 times 10^-2 moles of Cl_2(g) and 0.121 moles of COCl_2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q_c, equals The reaction must run in the forward direction to reach equilibrium. must run in...
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at 298 K. Delta G degree (NO_2(g)) = 51.84 kJ/mol, Delta G degree (N_2 O_4 (g)) = 98.28 kJ/mol. Calculate Delta G at 298 K if the partial pressures of NO_2 and N_2O_4 are 0.37 atm and 1.62 atm, respectively. Express your answer using one significant figure.
Consider the following reaction between carbon monoxide and hydrogen, CO(g) + 2 H_2(g) Equilibrium CH_3OH(l) K_p = 2.25 times 10^4 Give the K_p expression for this reaction Determine the equilibrium pressure of CO if the P(H_2) at equilibrium = 0.52 atm If the Q_p for a particular reaction mixture was measure as 2.30 times 10^-4, how will this reaction proceed?
The following reaction is performed at a certain temperature and these data are acquired. Please use the reaction and data to answer the NEXT 2 QUESTIONS: NO_2 (g) + H_2 O_2 (aq) NO_3 (g) + H_2 O (g); Delta H = -16.15 KJ/mol; K_c = 144 If a scientist observes this reaction at the same temperature starting with 4 M of NO_2 and 4 M of H_2 O_2, what will be the final concentration of NO_3? A. 0.7 M B....
Suppose a reaction occurs with the following mechanism: Step 1: 2AD Step 2: D+E- (fast) B+C (slow) 1. What is the overall reaction? [Select] 2. What is the intermediate in the mechanism? (Select] 3. What is the molecularity of step 1? (Select 4. Which step is the rate determining step? [Select) 5. What is the rate law predicted by this mechanism? [Select) Question 22 15 pts Consider the following reaction at equilibrium: CO(g) + 2H2(g) CH2OH(g) AH=-18 kJ How will...
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