The gas phase reaction of nitric oxide, NO, with bromine, Br2, to produce nitrosyl bromide, NOBr,
occurs according to the net reaction: A possible reaction mechanism is:
?1
Step 1: 2 NO ⇌ N2O2
?−1
Step 2: N2O2 + Br2
2NO+Br2 → 2NOBr
2 NOBr
Neither step is faster than the other. What is the order of the overall reaction, and what is the overall rate constant (expressed in terms of the individual rate constants for the elementary steps)?
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The gas phase reaction of nitric oxide, NO, with bromine, Br2,
to produce nitrosyl bromide, NOBr,...
Question 20 2.5 pts The gas-phase reaction of nitric oxide (NO) with bromine (Br2), occurs by...
Question 20 2.5 pts The gas-phase reaction of nitric oxide (NO) with bromine (Br2), occurs by the following two- step mechanism: NO(g) + NO(g) = N2O2(g) (fast, equilibrium) N202 + Br2 → 2 NOBr(g) (slow) What is the observed rate law for the overall reaction? A. Rate = k[NO] [N202][Br2] B. Rate = k[N202][Br] C. Rate = k[NO]”[Br2] D. Rate = k[NO] E. Rate = k[NO]”[N202][Br2]
Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data...
Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data for the initial rate of appearance of NOBr were obtained: Experiment [NO](M) [Br2](M) Initial Rate of Appearance of NOBr(M/s) 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 What is the rate of disappearance of Br2 when [NO]= 8.1×10−2 M and [Br2]= 0.22 M ? Express your answer using two significant figures.
References Nitrogen monoxide, NO, reacts with bromine, Br2, to give nitrosyl bromide, NOBr. 2NO(g) + Bra(9)...
References Nitrogen monoxide, NO, reacts with bromine, Br2, to give nitrosyl bromide, NOBr. 2NO(g) + Bra(9) - 2N0Br(9) A sample of 3.74 x 10-2 mol NO with 3.11 x 10-2 mol Br2 gives an equilibrium mixture containing 2.31 x 10-2 mol NOBr. What is the composition of the equilibrium mixture? mol NO mol Br2 mol NOB Submit Answer Try Another Version 7 item attempts remaining
8. Nitrosyl bromide (NOBr) decomposes to nitrogen oxide and bromine. Use the following data to determine...
8. Nitrosyl bromide (NOBr) decomposes to nitrogen oxide and bromine. Use the following data to determine the order of the decomposition reaction. time 6 12 18 24 INOBr] 0.0286 0.0253 0.0229 0.0208 0.0190 Ln NOB] -3.554 1 -3.677 -3.777 -3.873 -3.963 1/[NOBr] 35.0 39.5 43.7 48.1 52.6
Nitric oxide reacts with fluorine in the gas phase to form FNO(g) 2 NO(g) + F2(g)...
Nitric oxide reacts with fluorine in the gas phase to form FNO(g) 2 NO(g) + F2(g) → 2 FNO(g) A kinetic study showed that the reaction mechanism consists of two elementary steps NO + NO ⇌ N2O2 fast N2O2 + F2 →2 FNO slow The overall order of the reaction is therefore
For the decomposition of nitrosyl bromide at 10 °C 2 NOBr(g)2NO) +Br2(g) the average rate of...
For the decomposition of nitrosyl bromide at 10 °C 2 NOBr(g)2NO) +Br2(g) the average rate of disappearance of NOBr over the time period from t-0s to t 6.48 s is found to be 2.24 102Ms What is the average rate of appearance of Br2 over the same time period? Submit Show Anproach Show Tutor Steps Sulbmit Answer 5 iten attempts remaining
Nitric oxide reacts with fluorine in the gas phase to form FNO(g) 2 NO(g) + F2(g)...
Nitric oxide reacts with fluorine in the gas phase to form FNO(g) 2 NO(g) + F2(g) → 2 FNO(g) A kinetic study showed that the reaction mechanism consists of two elementary steps NO + NO ⇌ N2O2 fast N2O2 + F2 →2 FNO slow The overall order of the reaction is therefore A. 2 B. 2.5 C. 1 D. 3 E. 1.5
Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: rate constant elementary...
Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: rate constant elementary reaction step NO(g)+ 02(g) NO2(9) 0(g) 1 NO(g) O(g) NO2(9) k2 2 Suppose also k,»k,. That is, the first step is much faster than the second. 2* Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical reaction rate k Note: your answer should not contain the concentrations of any intermediates. Express the rate...
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...
What is the rate of disappearance of Br2 when [NO]= 8.6×10−2 M and [Br2]= 0.31 M...
What is the rate of disappearance of Br2 when [NO]= 8.6×10−2 M and [Br2]= 0.31 M ? Express your answer using two significant figures. The rate of disappearance of Br2 is half the rate of appearance of NOBr, and the initial problem was: Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data for the initial rate of appearance of NOBr were obtained: Experiment [NO](M) [Br2](M) Initial Rate of Appearance of NOBr(M/s) 1 0.10...
Question 20 2.5 pts The gas-phase reaction of nitric oxide (NO) with bromine (Br2), occurs by the following two- step mechanism: NO(g) + NO(g) = N2O2(g) (fast, equilibrium) N202 + Br2 → 2 NOBr(g) (slow) What is the observed rate law for the overall reaction? A. Rate = k[NO] [N202][Br2] B. Rate = k[N202][Br] C. Rate = k[NO]”[Br2] D. Rate = k[NO] E. Rate = k[NO]”[N202][Br2]
References Nitrogen monoxide, NO, reacts with bromine, Br2, to give nitrosyl bromide, NOBr. 2NO(g) + Bra(9) - 2N0Br(9) A sample of 3.74 x 10-2 mol NO with 3.11 x 10-2 mol Br2 gives an equilibrium mixture containing 2.31 x 10-2 mol NOBr. What is the composition of the equilibrium mixture? mol NO mol Br2 mol NOB Submit Answer Try Another Version 7 item attempts remaining
8. Nitrosyl bromide (NOBr) decomposes to nitrogen oxide and bromine. Use the following data to determine the order of the decomposition reaction. time 6 12 18 24 INOBr] 0.0286 0.0253 0.0229 0.0208 0.0190 Ln NOB] -3.554 1 -3.677 -3.777 -3.873 -3.963 1/[NOBr] 35.0 39.5 43.7 48.1 52.6
For the decomposition of nitrosyl bromide at 10 °C 2 NOBr(g)2NO) +Br2(g) the average rate of disappearance of NOBr over the time period from t-0s to t 6.48 s is found to be 2.24 102Ms What is the average rate of appearance of Br2 over the same time period? Submit Show Anproach Show Tutor Steps Sulbmit Answer 5 iten attempts remaining
Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: rate constant elementary reaction step NO(g)+ 02(g) NO2(9) 0(g) 1 NO(g) O(g) NO2(9) k2 2 Suppose also k,»k,. That is, the first step is much faster than the second. 2* Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical reaction rate k Note: your answer should not contain the concentrations of any intermediates. Express the rate...
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