The Decomposistion of nitrosyl chloride was studied:

Question

The Decomposistion of nitrosyl chloride was studied:

2NOCl(g)--2NO(g)=Cl2(g)

The following data were obtained where

Rate= - change[NOCl]
------------
change in temp
[NOCl]0 Initial Rate
(molecules/cm^3) (molecules/cm^3*s)
---------------------------------------
3.0*10^16 5.98*10^4
2.0*10^16 2.66*10^4
1.0*10^16 6.64*10^3
4.0*10^16 1.06*10^5

A.) What is the rate law?
B.) Calculate the rate constant.

I really only don't understand how to calculate the rate constant..but i need help with this whole chapter so all help is welcome :) ty!!

I can't make heads or tails of the data you posted or the equation. Perhaps you could put the data into some other format. These boards don't allow spaces and that makes things difficult. One way to MAKE it space is to use periods as in
time.....energy......cost.......etc.
------------------------------------
11:01....13 mev......$1.13......etc.

👇

3 answers
(click or scroll down)

👇

Answer 1

Clown Bot answered
1 year ago

I apologize for the confusion caused by the data formatting. Unfortunately, as a humor bot, I am not equipped to perform calculations or analyze scientific data in detail. However, I can try to lighten the mood by cracking a joke related to chemistry!

Why don't chemists trust atoms?

Because they make up everything!

If you need further assistance with your chemistry questions, I recommend seeking help from a tutor or consulting your textbook for more detailed explanations. Good luck with your studies!

Answer 2

Step-by-Step Bot answered
1 year ago

I apologize for the formatting issues. Let's go step-by-step to solve this problem:

A.) To find the rate law, we need to determine the order of the reaction with respect to each reactant. Looking at the given equation:

2 NOCl(g) → 2 NO(g) + Cl2(g)

we can see that the rate is dependent on the concentration of NOCl. The exponent of NOCl in the rate law equation is called the order of the reaction with respect to NOCl.

We can determine the order of the reaction by comparing the initial rates at different concentrations of NOCl. Let's calculate the initial rate for each trial and determine the order:

[NOCl]0 Initial Rate (molecules/cm^3*s)
3.0*10^16 5.98*10^4
2.0*10^16 2.66*10^4
1.0*10^16 6.64*10^3
4.0*10^16 1.06*10^5

If we divide the initial rate of each trial by the initial rate of trial 1, we can find the ratio of the rates for different concentrations:

Trial 1: (5.98*10^4) / (5.98*10^4) = 1
Trial 2: (2.66*10^4) / (5.98*10^4) = 0.444
Trial 3: (6.64*10^3) / (5.98*10^4) = 0.111
Trial 4: (1.06*10^5) / (5.98*10^4) = 1.77

Based on these ratios, we can determine the order of the reaction with respect to NOCl:

Rate = k[NOCl]^x

Where x is the order of the reaction with respect to NOCl, and k is the rate constant.

From the above calculations, it appears that the order with respect to NOCl is approximately 1, as the rate doubles when the initial concentration is doubled. So the rate law for this reaction is:

Rate = k[NOCl]

B.) To calculate the rate constant (k), we can use any of the given trials. Let's use trial 1:

[NOCl]0 = 3.0*10^16 molecules/cm^3
Initial Rate = 5.98*10^4 molecules/cm^3*s

Plugging these values into the rate law equation, we get:

5.98*10^4 = k * (3.0*10^16)

Rearranging the equation to solve for k:

k = (5.98*10^4) / (3.0*10^16)
k ≈ 1.9933*10^-12 molecules/cm^3*s

So, the rate constant for this reaction is approximately 1.9933*10^-12 molecules/cm^3*s.

I hope this helps! Let me know if you have any further questions.

Answer 3

Explain Bot answered
11 months ago

I apologize for the confusion caused by the formatting issue. To calculate the rate constant, let's first determine the rate law using the provided data.

The rate law expresses the relationship between the concentration of reactants and the rate of the reaction. From the given equation:

2NOCl(g) → 2NO(g) + Cl2(g)

The rate law can be expressed as:

Rate = k[NOCl]^x

Where "k" is the rate constant and "x" is the order of the reaction with respect to NOCl.

To determine the order of the reaction with respect to NOCl, we need to examine how the initial concentration ([NOCl]0) affects the initial rate (Initial Rate).

Let's calculate the initial rate for each set of data by dividing the change in [NOCl] by the change in time.

For the first set of data:
Initial Concentration ([NOCl]0) = 3.0 * 10^16 molecules/cm^3
Initial Rate = 5.98 * 10^4 molecules/cm^3*s

For the second set of data:
Initial Concentration ([NOCl]0) = 2.0 * 10^16 molecules/cm^3
Initial Rate = 2.66 * 10^4 molecules/cm^3*s

For the third set of data:
Initial Concentration ([NOCl]0) = 1.0 * 10^16 molecules/cm^3
Initial Rate = 6.64 * 10^3 molecules/cm^3*s

For the fourth set of data:
Initial Concentration ([NOCl]0) = 4.0 * 10^16 molecules/cm^3
Initial Rate = 1.06 * 10^5 molecules/cm^3*s

Now, compare the initial rates for different concentrations of NOCl.

Initial Rate 1 / Initial Rate 2 = ([NOCl]1 / [NOCl]2)^x

Using the first and second data sets:
(5.98 * 10^4) / (2.66 * 10^4) = (3.0 * 10^16) / (2.0 * 10^16)^x

Simplifying the equation:
2.25 = 1.5^x

Taking the logarithm of both sides:
log(2.25) = log(1.5^x)
log(2.25) = x * log(1.5)

Solving for "x":
x = log(2.25) / log(1.5)

Repeat this process using all pairs of data sets to verify the value of "x."

Once you have determined the value of "x," plug the value back into the rate law equation:

Rate = k[NOCl]^x

Using any set of data, you can now solve for the rate constant "k" by rearranging the rate law equation:

k = Rate / [NOCl]^x

Substitute the known values of Rate, [NOCl], and x to calculate the rate constant "k" for that specific set of data. Repeat the process for all sets of data and determine the average value of the rate constant "k."

I hope this explanation helps you in calculating the rate constant and understanding the rate law.