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2. A reaction D+B products is found to be zeroth...
please help with these two questions The following data were obtained for the formation of nitrosyl...
please help with these two questions
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine. Initial (NO) Initial (Bra) Initial rate of reaction Trial 1 0.025 M 0.040 M 1.2 m/s Trial 20.025 M 0.080 M 2.4 M/S Trial 3 0.025 M 0.120 M 3.6 M/s Trial 4 0.050 M 0.040 M 4.8 M/s Trial 5 0.075 M 0.040 M 10.8 Mis The rate law for this reaction would be: zero-order in NO...
I need help please: Reaction Mechanisms and Catalysis 1. The rate constant in an elementary reaction's...
I
need help please: Reaction Mechanisms and Catalysis
1. The rate constant in an elementary reaction's rate equation can be modeled by the Arrhenius equation: & Ae a. The coefficient A is the frequency factor. What are the units of A for a first-order reaction? Justify your answer mathematically. (2 points) b. Describe how the value of A is affected by molecular collisions. (1 point) c. Is the effect of the reaction temperature on A high, low, or moderate? Explain....
1) 2) 3) A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step...
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A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) N20(g) + H20(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) +H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO2 Ok[NO]2[H212 O k[NO]2[H2] Ok[N20][H2] k[NO]1/2[H2] 2NO(g) +Cl2 (g) → NOCI (8) Experiment concentration of NO (M) 0.09 0.045 0.045 concentration of Cl2(M) Rate (M/s) 0.01 3.40 x 10-4 8.50 x...
Please help i need to get these right in order to get an A PLEASE PLEASE...
Please help i need to get these right in order to get an A PLEASE PLEASE PLEASE 1. What is the Kc for the following reaction at equilibrium at 1000 ∘C if [CO]= 0.50 M , [H2]= 0.32 M , [CH4]= 1.6 M , and [H2O]= 2.8 M ? CO(g)+3H2(g)⇌CH4(g)+H2O(g) 2. The equilibrium constant, Kc, for the reaction of H2 and N2 is 1.7×102 at 225 ∘C. 3H2(g)+N2(g)←−→2NH3(g) If the system at equilibrium contains 0.19 M H2 and 0.026 M...
Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300...
Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300 °C Part 2. Given the initial conditions below, in which direction is the reaction expected to proceed? [N2] = 0.015 M [H2] = 0.010 M [NH3] = 0.025 M a neither, the reaction is at equilibrium O b. to the right c. to the left Which of the following acidic solutions has the lowest pH? O a. 0.10 M HMO pka = 8.23 O...
The second-order reaction, 2 Mn(CO)_5 rightarrow Mn_2 (CO)_10 is found to have a rate constant equal...
The second-order reaction, 2 Mn(CO)_5 rightarrow Mn_2 (CO)_10 is found to have a rate constant equal to 512 M^-1 S^-1. If the initial concentration of Mn(CO)_5 is 0.011 M, how long will it take for the reactant concentration to reach 0.0011 M? Units: s a. 1.6 b. 5.1 c. 0.020 d. 0.28 A plot of a 1/[A] versus time gave a straight line. This indicates that A rightarrow B + C a. the reaction is zero order in reagent A...
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related...
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
14. A catalyst a. Participates in the reaction and b. Dec c. Increases the activation e...
14. A catalyst a. Participates in the reaction and b. Dec c. Increases the activation e d. Binds to the reactants and releases them sequentially the reaction and changes the product release reases the activation energy required for the reaction 15. In an exothermic reaction, if heat is removed from the reaction a. Equilibrium shifts to the right b. Product formation increases c. Increase the value of K d. All the above 16. Initially, a mixture of 0.100 M No,...
10. Consider the reaction A + 2B → C ne rate law for this reaction is...
10. Consider the reaction A + 2B → C ne rate law for this reaction is on der in and and order in B if the rate constant at 25°C is 1.25x 105 , find the rate of reaction when the concentration of A is 0.27M and the concentration of B is 0.32 M UMA 21 11. Consider the reaction A +2B C + D. The rate law for this reaction is first order in A and zeroth order in...
1) 2) 3) The slope and intercept of an Arrhenius plot made for the first-order decomposition...
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The slope and intercept of an Arrhenius plot made for the first-order decomposition reaction are -2864.3 K and 23.279 at 303K, what is the value of the activation energy (KJ/mol) at this temperature? The value of Keq for the following reaction is 0.340: A (g) +B (g)=C(g) +D (g) The value of Keq at the same temperature for the reaction below is 3C (g) + 3D (g) = 3A (g) + 3B (g) 2NO(g) +Cl2 (g) →...
please help with these two questions
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine. Initial (NO) Initial (Bra) Initial rate of reaction Trial 1 0.025 M 0.040 M 1.2 m/s Trial 20.025 M 0.080 M 2.4 M/S Trial 3 0.025 M 0.120 M 3.6 M/s Trial 4 0.050 M 0.040 M 4.8 M/s Trial 5 0.075 M 0.040 M 10.8 Mis The rate law for this reaction would be: zero-order in NO...
I
need help please: Reaction Mechanisms and Catalysis
1. The rate constant in an elementary reaction's rate equation can be modeled by the Arrhenius equation: & Ae a. The coefficient A is the frequency factor. What are the units of A for a first-order reaction? Justify your answer mathematically. (2 points) b. Describe how the value of A is affected by molecular collisions. (1 point) c. Is the effect of the reaction temperature on A high, low, or moderate? Explain....
1)
2)
3)
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) N20(g) + H20(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) +H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO2 Ok[NO]2[H212 O k[NO]2[H2] Ok[N20][H2] k[NO]1/2[H2] 2NO(g) +Cl2 (g) → NOCI (8) Experiment concentration of NO (M) 0.09 0.045 0.045 concentration of Cl2(M) Rate (M/s) 0.01 3.40 x 10-4 8.50 x...
Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300 °C Part 2. Given the initial conditions below, in which direction is the reaction expected to proceed? [N2] = 0.015 M [H2] = 0.010 M [NH3] = 0.025 M a neither, the reaction is at equilibrium O b. to the right c. to the left Which of the following acidic solutions has the lowest pH? O a. 0.10 M HMO pka = 8.23 O...
The second-order reaction, 2 Mn(CO)_5 rightarrow Mn_2 (CO)_10 is found to have a rate constant equal to 512 M^-1 S^-1. If the initial concentration of Mn(CO)_5 is 0.011 M, how long will it take for the reactant concentration to reach 0.0011 M? Units: s a. 1.6 b. 5.1 c. 0.020 d. 0.28 A plot of a 1/[A] versus time gave a straight line. This indicates that A rightarrow B + C a. the reaction is zero order in reagent A...
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
14. A catalyst a. Participates in the reaction and b. Dec c. Increases the activation e d. Binds to the reactants and releases them sequentially the reaction and changes the product release reases the activation energy required for the reaction 15. In an exothermic reaction, if heat is removed from the reaction a. Equilibrium shifts to the right b. Product formation increases c. Increase the value of K d. All the above 16. Initially, a mixture of 0.100 M No,...
10. Consider the reaction A + 2B → C ne rate law for this reaction is on der in and and order in B if the rate constant at 25°C is 1.25x 105 , find the rate of reaction when the concentration of A is 0.27M and the concentration of B is 0.32 M UMA 21 11. Consider the reaction A +2B C + D. The rate law for this reaction is first order in A and zeroth order in...
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2)
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The slope and intercept of an Arrhenius plot made for the first-order decomposition reaction are -2864.3 K and 23.279 at 303K, what is the value of the activation energy (KJ/mol) at this temperature? The value of Keq for the following reaction is 0.340: A (g) +B (g)=C(g) +D (g) The value of Keq at the same temperature for the reaction below is 3C (g) + 3D (g) = 3A (g) + 3B (g) 2NO(g) +Cl2 (g) →...
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