Question

Select all that apply. The rate law for the reaction 2NO(g) + Cl2(g) → 2NOCl(g) is...

Select all that apply.

The rate law for the reaction

2NO(g) + Cl2(g)

2NOCl(g)

is given by R = k[NO][Cl2]

If the following is the mechanism for the reaction,

NO(g) + Cl2(g)

NOCl2(g)

NOCl2(g) + NO(g)

2NOCl(g)

which of the following statements accurately describes this reaction? Check all that apply.
  

2nd order reaction

  

The first step is the slow step.

  

Doubling [NO] would quadruple the rate.

  

Cutting [Cl2] in half would decrease the rate by a factor of two.

  

The molecularity of the first step is 1.

  

Both steps are termolecular.

Homework Answers

Answer #1

I have not included in the attached sheet by mistake but explanation is there.

The molecularity of the first step is 1 ------------------------Correct

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the reaction between NO and Cl2 to form NOCl: 2NO(g)+Cl2(g)⇌2NOCl(g) A reaction mixture at a...
Consider the reaction between NO and Cl2 to form NOCl: 2NO(g)+Cl2(g)⇌2NOCl(g) A reaction mixture at a certain temperature initially contains only [NO]= 0.50 M and [Cl2]= 0.55. After the reaction comes to equilibrium, the concentration of NOCl is 0.35 M . Part A Find the value of the equilibrium constant (Kc) at this temperature. Express your answer using two significant figures. Kc=???
The reaction 2NOCl(g) 2NO(g) + Cl2(g) has an equilibrium constant Kp (in terms of pressures) at...
The reaction 2NOCl(g) 2NO(g) + Cl2(g) has an equilibrium constant Kp (in terms of pressures) at 300 °C of 0.180. Calculate the concentration of NO that will be present at 300 °C in equilibrium with NOCl (at a concentration of 1.89×10-2 mol L-1) and Cl2 (at a concentration of 7.00×10-3 mol L-1). [NO] =    mol L-1
Consider this initial-rate data at a certain temperature for the reaction described by: 2NOCl(g) yields 2NO(g)...
Consider this initial-rate data at a certain temperature for the reaction described by: 2NOCl(g) yields 2NO(g) + Cl2(g) NOCl                                Intl. Rate of Form. of Cl2 (M) .600                                   1.46 x 10^-5 .750                                   2.28 x 10^-5 .900                                    3.28 x 10^-5 Determine the value and units of the rate constant. k=
The experimentally determined rate law for the reaction 2NO(g)+2H2(g)→N2(g)+2H2O(g) is rate=k[NO]2[H2]. Part A What are the...
The experimentally determined rate law for the reaction 2NO(g)+2H2(g)→N2(g)+2H2O(g) is rate=k[NO]2[H2]. Part A What are the reaction orders in this rate law? Enter your answers numerically separated by commas. nNO, nH2 = SubmitMy AnswersGive Up Part B Would the reaction rate increase more if we double the concentration of NO or the concentration of H2? A) The reaction rate will increase more if we double the concentration of NO. B) The reaction rate will increase more if we double the...
1. For the reaction: 2NOCl(g) 2NO(g) + Cl2(g), Kc = 1.6 x 10− 5 . What...
1. For the reaction: 2NOCl(g) 2NO(g) + Cl2(g), Kc = 1.6 x 10− 5 . What are the equilibrium concentrations of each species if 1.0 mole of NOCl is initially placed in an empty 2.0 L flask? 2. A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H2(g) + I2(g): When the system comes to equilibrium at 425 °C, PHI = 0.708 atm and 2 2 P P H I =...
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow NO2(g)+Cl(g)→ClNO2(g)Fast Part A What is the overall...
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow NO2(g)+Cl(g)→ClNO2(g)Fast Part A What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Identify the intermediates in the mechanism Part C What is the predicted rate law?
Using the reaction mechanism given below write a rate expression for the reaction shown. Reaction: COCl2(g)...
Using the reaction mechanism given below write a rate expression for the reaction shown. Reaction: COCl2(g) + Cl2(g) → CO(g) + 2 Cl2 (g) Mechanism: Step 1 Cl2 (g) ↔ 2 Cl (g) fast Step 2 Cl (g) +COCl2 (g) → COCl (g) + Cl2 (g) slow Step 3 COCl (g) + Cl (g) ↔ CO (g) + Cl2 (g) fast rate = ?
The rate law for the reaction: 2H2+2NO--->N2+2H2O is rate=k[H2][NO]^2. Which of the follwing mechanisms can be...
The rate law for the reaction: 2H2+2NO--->N2+2H2O is rate=k[H2][NO]^2. Which of the follwing mechanisms can be ruled out on the basis of the observed rate expression? PLEASE EXPLAIN Mechanism 1: H2+NO--->H2O+N (slow) / N+NO----->N2+O (fast) / O+H2----> N2+O (fast) Mechanism 2: H2+2NO---->N2O+H2O (slow) / N2O+H2---->N2+H2O (fast) Mechanism 3: 2NO<----->N2O2 (fast equilibrium) / N2O2+H2------>N2O+H2O (slow) / N2O+H2------>N2+H2O (fast) PLEASE EXPLAIN WHY.
Using the reaction mechanism given below write a rate expression for the reaction shown. Reaction: COCl2(g)...
Using the reaction mechanism given below write a rate expression for the reaction shown. Reaction: COCl2(g) + Cl2(g) → CO(g) + 2 Cl2 (g) Mechanism: Step 1 Cl2 (g) ↔ 2 Cl (g) fast Step 2 Cl (g) +COCl2 (g) → COCl (g) + Cl2 (g) slow Step 3 COCl (g) + Cl (g) ↔ CO (g) + Cl2 (g) fast rate = ? I think the rate should be k2 [Cl] [COCl2] but I'm not sure if that's right.
1. The rate law for the reaction is: Cl2(g) + CHCl3 (g) = HCl (g) +...
1. The rate law for the reaction is: Cl2(g) + CHCl3 (g) = HCl (g) + CCl4 (g) Is Rate = k [Cl2]^1/2 [CHCl3] What are the units for k, assuming time inow seconds and concentration in mol/L 2. What is the unit for the rate of a chemical reaction and the rate constant for a third-order rate law?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT