2NOBr(g) rightarrow 2NO(g) + Br2(g) [NOBr] (mol L^- 1) 0.0450 0.0310 0.0095 Rate (mol L^- 1...
QUESTION 6 2NOBr(g) → 2NO(g) + Br2(g) [NOB:](mol =) Rate (mol-1,-1) 0.0450 162 * 10-3 0.0310 7.69 x 10-4 0.0095 7.22 x 10-5 Based on the initial rate data above, what is the value of the rate constant? 20.0360 L mol's- ob-0.800L mol-'s-1 C 1.25 L mor-15-1 od 278 L mol-1-1 € 0.0360s-1
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. Please help:) 52. For the reachon ZNO Brly) - 2Noig) + Brela) the rate of the reaction was -23 mol NoBrilh when the inihol NOBY Coventration was 2 mol NOBYL Wat is the rate constant of the reaction?
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 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.
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) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 89 s. M
The rate equation for the reaction 2NO(g) + Br_2(g) rightgarrow 2NOBr(g) was determined experimentally to be: Rate = k[NO]^2 [Br_2] Five possible mechanisms have been proposed (i)-(v). Determine the rate equation for each mechanism below and then decide with reasons, (based on the information given) which mechanism is the most likely. (i) 2NO (g) + Br_2 (g) rightarrow 2NOBr (g) (ii)NO (g) + Br_2 rightwardsharpoonoverleftwardsharpoon NOBr_2 (g) NOBr_2 (g) + NO (g) rightarrow 2NOBr (g) (iii) Br_2 rightwardsharpoonoverleftwardsharpoon Br +...
2NOBr(g)(double arrow)2NO(g) + Br2(g) If 0.382 moles of NOBr(g), 0.517 moles of NO, and 0.579 moles of Br2 are at equilibrium in a 17.5L container at 522 K, the value of the equilibrium constant, Kc, is
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 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...