lthe system 2NO (g) +Cl2 (g) <-----> 2 NOCl (g) has a Kc= 6.5x10^4 at 35°C....
lthe system 2NO (g) +Cl2 (g) <-----> 2 NOCl (g)
has a Kc= 6.5x10^4 at 35°C. determine which direction will the
system shift (forward or backward) if it has these initial
concentrations:
[NO]0 =0.0275 M, [Cl2]0 =0.0384 M, [NOCl]0 =1.750 M.
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lthe system 2NO (g) +Cl2 (g) <-----> 2 NOCl (g)
has a Kc= 6.5x10^4 at 35°C....
The initial concentrations or pressures of reactants and products are given for each of the following...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (d) 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) KP = 16.5; initial pressures: SO3 = 1.00 atm, SO2 = 1.00 atm, O2 = 1.00 atm (e) 2NO(g) + Cl2 (g) ⇌ 2NOCl(g) Kc = 4.6 × 104 ; [NO] = 1.00 M, [Cl2] = 1.00...
For the following reaction: 2NOCl(g) → 2NO(g) + Cl2(g) determine: a) the differential rate...
For the following reaction: 2NOCl(g) → 2NO(g) + Cl2(g) determine: a) the differential rate law b) the integrated rate law c) the value for the rate constant d) the concentration of NOCl(g) remaining after 275 s in each trial given: Trial [NOCl]0 (mol/L) Initial Rate (mol/L•s) 1 3.15 7.88 × 10–3 2 6.30 1.57 × 10–2 3 12.6 3.15 × 10–2
1) 2) 3) 2NO(g) +Cl2 (g) → NOCI (8) Experiment concentration of NO (M) 0.09 0.045...
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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 10-5 0.04 3.40 x 10-4 0.01 What is the reaction order with respect to NO to Cl2 ? overall reaction order ? the reaction order with respect to reaction order ? what is the rate constant * All orders are integers * Rate constant: Please report 3 significant figures. Numbers only, No...
The initial concentrations or pressures of reactants and products are given for each of the following...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. 2NH3(g)⇌N2(g)+3H2(g)Kc=17; [NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M (b) 2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104; NH3 = 3.0 atm, N2 = 2.0 atm, H2 = 1.0 atm (c) 2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230; [SO3] = 0.00 M, [SO2] = 1.00 M, [O2] = 1.00 M (d) 2SO3(g)⇌2SO2(g)+O2(g)KP=16.5; SO3 = 1.00...
At high temperatures, Cl2 breaks down into chlorine atoms: Cl2 (g)⇌ 2 Cl (g) If Kc...
At high temperatures, Cl2 breaks down into chlorine atoms: Cl2 (g)⇌ 2 Cl (g) If Kc =2.68 at a given temperature, find the equilibrium concentrations of Cl2 and Cl if the initial concentration of Cl2 is 1.05 M. Answers: A. [Cl2] = 0.201 M, [Cl] = 1.85 M B. [Cl2] = 0.444 M, [Cl] = 0.799 M C. [Cl2] = 0.288 M, [Cl] = 0.532 M D. [Cl2] = 0.482 M, [Cl] = 1.14 M
The equilibrium constant, K, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g)...
The equilibrium constant, K, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g) + Cl2(8) = 2NOCI(g) is 6.5 x 104 at 35°C. In which direction will the reaction proceed to reach equilibrium if the starting concentrations of NO, Cl., and NOCI are 2.6 x 10-3 M, 7.4 x 10-M, and 5.8 M respectively? o o O shift right shift lent neither
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...
consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) At a given point in a reaction, [SO2Cl2] = 0.12 M,...
consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) At a given point in a reaction, [SO2Cl2] = 0.12 M, [Cl2] = 0.16 M and [SO2] = 0.050 M. Kc = 0.078. Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to reach equilibrium?
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a...
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a certain temperature, the equilibrium concentrations are [NO]-0.31 M [H2]-0.16 M [N2] 0.082 M and [H:0]-4.64 M (a) Write the equilibrium expression for the reaction. (b) Determine the value of the equilibrium constant 2. The equilibrium constant Kc for the following reaction is 150.7 at 1 15°C: 12 (g) + Br2 (g) ←→ 2 IBr(g) 2.00 moles of each gas (l2, Br: and IBr) are...
QUESTION 2 CO(g) + Cl2(g) = COCI_(a) Kc - 1.2 x 10 at 400 °C Consider...
QUESTION 2 CO(g) + Cl2(g) = COCI_(a) Kc - 1.2 x 10 at 400 °C Consider the above reaction. If the (CO) = [C12] = [COC12] = 5 x 10-6 M at some point during the reaction, is the reaction at equilibrium? If not, in which direction will the reaction proceed in order to reach equilibrium? Use the Math Editor to show your work or complete on paper and upload in the next quesiton. 1. Calculate 2. Is Q> or...
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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 10-5 0.04 3.40 x 10-4 0.01 What is the reaction order with respect to NO to Cl2 ? overall reaction order ? the reaction order with respect to reaction order ? what is the rate constant * All orders are integers * Rate constant: Please report 3 significant figures. Numbers only, No...
The equilibrium constant, K, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g) + Cl2(8) = 2NOCI(g) is 6.5 x 104 at 35°C. In which direction will the reaction proceed to reach equilibrium if the starting concentrations of NO, Cl., and NOCI are 2.6 x 10-3 M, 7.4 x 10-M, and 5.8 M respectively? o o O shift right shift lent neither
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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...
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a certain temperature, the equilibrium concentrations are [NO]-0.31 M [H2]-0.16 M [N2] 0.082 M and [H:0]-4.64 M (a) Write the equilibrium expression for the reaction. (b) Determine the value of the equilibrium constant 2. The equilibrium constant Kc for the following reaction is 150.7 at 1 15°C: 12 (g) + Br2 (g) ←→ 2 IBr(g) 2.00 moles of each gas (l2, Br: and IBr) are...
QUESTION 2 CO(g) + Cl2(g) = COCI_(a) Kc - 1.2 x 10 at 400 °C Consider the above reaction. If the (CO) = [C12] = [COC12] = 5 x 10-6 M at some point during the reaction, is the reaction at equilibrium? If not, in which direction will the reaction proceed in order to reach equilibrium? Use the Math Editor to show your work or complete on paper and upload in the next quesiton. 1. Calculate 2. Is Q> or...
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