The reaction between nitric oxide (NO) and chlorine (Cl2) to form nitrosyl chloride (NOCl) was found...
The reaction between nitric oxide (NO) and chlorine (Cl2) to form nitrosyl chloride (NOCl) was found to occur as an elementary reaction as follows:
2 NO (g) + Cl2 (g) à 2 NOCl (g)
A table of the concentrations and initial rates data is shown below:
[ NO ]0 (M) [ Cl2 ]0 (M) rate = - D[Cl2]/ Dt (M / min)
Run 1 0.10 0.10 0.18
Run 2 0.10 0.20 0.36
Run 3 0.20 0.20 1.44
The order for Cl2 in this reaction is:
(a) 1 (b) 45 (c) 2 (d) 180
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The reaction between nitric oxide (NO) and chlorine
(Cl2) to form nitrosyl chloride (NOCl) was found...
Nitric oxide reacts with chlorine to form nitrosyl chloride, NOCl. Use the following data to determine...
Nitric oxide reacts with chlorine to form nitrosyl chloride, NOCl. Use the following data to determine the rate equation for the reaction. NO + 1/2Cl2 --> NOCl Expt. # [NO] [Cl2] Initial Rate 1 0.22 0.065 0.96 M/min 2 0.66 0.065 8.6 M/min 3 0.44 0.032 1.9 M/min Would someone provide a solution with detailed step?
PLEASE ANSWER BOTH QUESTIONS PLEASE ! 19. (5 pts.) At 79.00°F the enthalpy of a reaction...
PLEASE ANSWER BOTH QUESTIONS PLEASE !
19. (5 pts.) At 79.00°F the enthalpy of a reaction was found to be +342.8 KJ/mole and its entropy change was +395.0 J/mole*K. The value of the Gibb's free energy is: (a) +341.0 KJ/mole (b)_-461.0 KJ/mole (C) -341.0 KJ/mole (d) +224.6 KJ/mole 20. (5 pts.) The reaction between nitric oxide (NO) and chlorine (Cl2) to form nitrosyl chloride (NOCI) was found to occur as an elementary reaction as follows: 2 NO (g) + Cl2...
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
Nitric oxide (NO) reacts with chlorine gas (Cl) to form nitrosyl chloride (NOC) according to the...
Nitric oxide (NO) reacts with chlorine gas (Cl) to form nitrosyl chloride (NOC) according to the reaction below: 2 NO(g) + C12()=2 NOCI(g) Kp = ? at 700 K A rigid vessel initially contains equimolar amounts of NO and C1, (and nothing else) at 700 K and a total pressure of 2.00 bar. After the system reaches equilibrium at 700 K, the total pressure is found to be 1.84 bar. What is the value of the equilibrium constant Kp? A)...
The compound NOCl decomposes to nitric oxide and chlorine according to the following equation: 2 NOCl...
The compound NOCl decomposes to nitric oxide and chlorine according to the following equation: 2 NOCl (g) → 2 NO (g) + Cl2 (g) Suppose that 0.730 mol NOCl is placed in a 2.00-L flask at a given temperature. When equilibrium has been established, it is found that the concentration of NO is 0.0906 M. Calculate the equilibrium constant for this reaction.
3. Nitric oxide, NO(g) reacts with chlorine gas, Cl2(g), in the reaction 2NO(g) + Cl2(g) →...
3. Nitric oxide, NO(g) reacts with chlorine gas, Cl2(g), in the reaction 2NO(g) + Cl2(g) → 2NOCIG) Initial rates of reaction are determined for various combinations of initial concentrations of reactants and recorded below; Trial Initial [NO] (mol/L) 0.10 0.10 0.20 Initial (C12] (mol/L) 0.10 0.20 0.20 Rate of production of NOCI (mol/L.s) 1.8 x 107 3.6 x 102 1.43 x 10" a) What is the rate law equation for the reaction? (1 mark) b) What is the rate-determining step?...
2 NO(g) + Cl2(g) → 2 NOCl(g) Initial Rate (M-min-1) 0.18 0.36 1.45 Exp. # |...
2 NO(g) + Cl2(g) → 2 NOCl(g) Initial Rate (M-min-1) 0.18 0.36 1.45 Exp. # | I | [NO, 0.10 0.10 0.20 [CI, 0.10 0.20 0.20 2 Determine the rate law and calculate k.
1. Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine: 2NO(g) + Cl2(g)...
1. Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine: 2NO(g) + Cl2(g) → 2NOCI(g) The following initial rates at a given temperature were obtained for the concentrations listed below. Experiment Initial Rate (mol:L-.h-1) [NO]. (mol.L-1 [Cl2]. (mol.L-1). 2.21 8.84 0.5 0.25 4.42 0.25 0.5 What is the experimental rate law? 0.25 0.25
In a study of the gas phase decomposition of nitrosyl chloride at 400 K NOCl(g)-NO(g) +...
In a study of the gas phase decomposition of nitrosyl chloride at 400 K NOCl(g)-NO(g) + ½ Cl2(g) the following data were obtained: [NOCI], M 5.48x10-2 2.74x10-2 1.37×10-2 6.85x10-3 seconds 3.80x104 1.14x10 2.66x105 Hint: It is not necessary to graph these data. The observed half life for this reaction when the starting concentration is 5.48×10-2 M is s and when the starting concentration is 2.74x10 M is S. Ms The average Δ(1/[NOCl) At from t-0 s to t-3.80x10" s is...
The gas phase reaction of nitric oxide, NO, with bromine, Br2, to produce nitrosyl bromide, NOBr,...
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)?
9....
PLEASE ANSWER BOTH QUESTIONS PLEASE !
19. (5 pts.) At 79.00°F the enthalpy of a reaction was found to be +342.8 KJ/mole and its entropy change was +395.0 J/mole*K. The value of the Gibb's free energy is: (a) +341.0 KJ/mole (b)_-461.0 KJ/mole (C) -341.0 KJ/mole (d) +224.6 KJ/mole 20. (5 pts.) The reaction between nitric oxide (NO) and chlorine (Cl2) to form nitrosyl chloride (NOCI) was found to occur as an elementary reaction as follows: 2 NO (g) + Cl2...
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
Nitric oxide (NO) reacts with chlorine gas (Cl) to form nitrosyl chloride (NOC) according to the reaction below: 2 NO(g) + C12()=2 NOCI(g) Kp = ? at 700 K A rigid vessel initially contains equimolar amounts of NO and C1, (and nothing else) at 700 K and a total pressure of 2.00 bar. After the system reaches equilibrium at 700 K, the total pressure is found to be 1.84 bar. What is the value of the equilibrium constant Kp? A)...
3. Nitric oxide, NO(g) reacts with chlorine gas, Cl2(g), in the reaction 2NO(g) + Cl2(g) → 2NOCIG) Initial rates of reaction are determined for various combinations of initial concentrations of reactants and recorded below; Trial Initial [NO] (mol/L) 0.10 0.10 0.20 Initial (C12] (mol/L) 0.10 0.20 0.20 Rate of production of NOCI (mol/L.s) 1.8 x 107 3.6 x 102 1.43 x 10" a) What is the rate law equation for the reaction? (1 mark) b) What is the rate-determining step?...
2 NO(g) + Cl2(g) → 2 NOCl(g) Initial Rate (M-min-1) 0.18 0.36 1.45 Exp. # | I | [NO, 0.10 0.10 0.20 [CI, 0.10 0.20 0.20 2 Determine the rate law and calculate k.
1. Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine: 2NO(g) + Cl2(g) → 2NOCI(g) The following initial rates at a given temperature were obtained for the concentrations listed below. Experiment Initial Rate (mol:L-.h-1) [NO]. (mol.L-1 [Cl2]. (mol.L-1). 2.21 8.84 0.5 0.25 4.42 0.25 0.5 What is the experimental rate law? 0.25 0.25
In a study of the gas phase decomposition of nitrosyl chloride at 400 K NOCl(g)-NO(g) + ½ Cl2(g) the following data were obtained: [NOCI], M 5.48x10-2 2.74x10-2 1.37×10-2 6.85x10-3 seconds 3.80x104 1.14x10 2.66x105 Hint: It is not necessary to graph these data. The observed half life for this reaction when the starting concentration is 5.48×10-2 M is s and when the starting concentration is 2.74x10 M is S. Ms The average Δ(1/[NOCl) At from t-0 s to t-3.80x10" s is...
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)?
9....
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