for the reaction 2NOBr(g)---- 2NO(g)+Br2(g) the rate of the reaction -2.3 mol NOBr/L/h when the initial NOBr concentration was 6.2 mol NoBr/L. what is the rate constant of the reaction.
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for the reaction 2NOBr(g)---- 2NO(g)+Br2(g) the rate of the reaction -2.3 mol NOBr/L/h when the initial...
2NOBr(g) rightarrow 2NO(g) + Br2(g) [NOBr] (mol L^- 1) 0.0450 0.0310 0.0095 Rate (mol L^- 1...
2NOBr(g) rightarrow 2NO(g) + Br2(g) [NOBr] (mol L^- 1) 0.0450 0.0310 0.0095 Rate (mol L^- 1 s^- 1) 1.62 times 10^-3 7.69 times 10^- 4 7.22 times 10^- 5 Based on the initial rate data above, what is the value of the rate constant? 27.8 L mol^-1 s^- 1 0.0360 s^- 1 0.800 L mol^- 1 s^- 1 0.0360 L mol^- 1 s^- 1 1.25 L mol^- 1 s^- 1
The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g) 2NO(g) + Br2(g)...
The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 11.1 L container at 298K contains 0.376 mol of NOBr(g) and 0.396 mol of NO, the equilibrium concentration of Br2
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s)...
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 59 s.
A student ran the following reaction in the laboratory at 295 K: 2NO(g) + Br2(g) <--->...
A student ran the following reaction in the laboratory at 295 K: 2NO(g) + Br2(g) <---> 2NOBr(g) When she introduced 0.153 moles of NO(g) and 0.123 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.117 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ____ The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g) <---> 2NO(g) + Br2(g) If an equilibrium mixture of...
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s)...
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 89 s. M
2NO(g) + Br2(g) = 2NOBr(g) Experiment [NO-] (M) [Br2] (M) Initial Rate (M s-1) 1 0.10...
2NO(g) + Br2(g) = 2NOBr(g) Experiment [NO-] (M) [Br2] (M) Initial Rate (M s-1) 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 1.) Determine the rate law equation for the reaction. 2.) What is the overall order of the reaction? 3.) What are the value and the units of the rate constant, k? 4.) Write the expression to show how is the rate of disappearance of bromine, Br2, related to the rate...
The equilibrium constant for the reaction: 2NO(g) + Br2(g)<----> 2NOBr(g) is Kc = 1.3x10^-2 at...
The equilibrium constant for the reaction: 2NO(g) + Br2(g) <----> 2NOBr(g) is Kc = 1.3x10^-2 at 1,000 Ka.) At this temperature, does the equilibrium favor the product or reactants?b.) Calculate Kc for 2NOBr <----> 2NO + Br2c.) Calculate Kc for NOBr <----> NO + 1/2Br2
A student ran the following reaction in the laboratory at 254 K: 2NO(g) + Br2(g) ⇌ 2NOBr(g)...
A student ran the following reaction in the laboratory at 254 K: 2NO(g) + Br2(g) ⇌ 2NOBr(g) When she introduced 0.185 moles of NO(g) and 0.130 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.152 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g)...
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 19.9 L container at 298K contains NOBr at a pressure of 0.297 atm and NO at a pressure of 0.251 atm, the equilibrium partial pressure of Br2 is ? atm.
5-10 The data below refer to the following reaction: 2NO(g) + Brz(g) 2NOBr(g) [NO] 2.5 [Brz] Concentration (M) Initial...
5-10 The data below refer to the following reaction: 2NO(g) + Brz(g) 2NOBr(g) [NO] 2.5 [Brz] Concentration (M) Initial Equilibrium [NOBr] 5.0 1.0 2.0 Calculate Kc Ans: 0.12 5-11 The AG of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions: O2(g) 52 0(g). A) 4.7 x 10-41 B) 2.3 x 10-61 C) 2.1 x 10-81 D) 2.1 x 1040 E) 4.5 x 1080
2NOBr(g) rightarrow 2NO(g) + Br2(g) [NOBr] (mol L^- 1) 0.0450 0.0310 0.0095 Rate (mol L^- 1 s^- 1) 1.62 times 10^-3 7.69 times 10^- 4 7.22 times 10^- 5 Based on the initial rate data above, what is the value of the rate constant? 27.8 L mol^-1 s^- 1 0.0360 s^- 1 0.800 L mol^- 1 s^- 1 0.0360 L mol^- 1 s^- 1 1.25 L mol^- 1 s^- 1
5-10 The data below refer to the following reaction: 2NO(g) + Brz(g) 2NOBr(g) [NO] 2.5 [Brz] Concentration (M) Initial Equilibrium [NOBr] 5.0 1.0 2.0 Calculate Kc Ans: 0.12 5-11 The AG of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions: O2(g) 52 0(g). A) 4.7 x 10-41 B) 2.3 x 10-61 C) 2.1 x 10-81 D) 2.1 x 1040 E) 4.5 x 1080
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