Question

If the rate of disappearance H2
= -0.13 M/s at a specific time, what is the value
for the rate of formation of HCl during the same interval?

Answer 1

This relationships depends on the mechanism. What is the chemical equation of the reaction you are analyzing?

Answer 2

H2 + 2 ICl  I2 + 2HCl…

Answer 3

Plz help me understand the concept

Answer 4

how will I find the value of rate?

Answer 5

Let's forget about rate for a second. If one mol of H2 has been reacted, how many moles of HCl is formed?

Answer 6

I dont know:(

Answer 7

2

Answer 8

as we can see in the product side

Answer 9

2HCL

Answer 10

That's right. Based on the coefficients, you know that each molecule (and mol) of H2 will go to form two molecules (and mol) HCl.

Answer 11

yes

Answer 12

So we can make an assumption that over any time interval, the ratio of H2 consumed to the ratio of HCl produced will be...

\[H_{2_{consumed}}:HCl_{produced}=1:2\]

Answer 13

Let's look back at the original problem now.

Answer 14

yes 1:2

Answer 15

If the rate of disappearance of H2 is -0.13M/s:\[Rate_{H_2}=-0.13\frac{M}{s} \]That means that every second, one M of H2 is being reacted. What does 1M mean in terms of moles?

Answer 16

the molecule of Hydrogen

Answer 17

that is disappeared every second and making two molecules of HCL

Answer 18

So if you have twice the number of molecules disappearing over the same time interval, what is the rate of disappearance of HCl?

Answer 19

1 mol

Answer 20

\[Rate=\frac{molecules}{t}\]

Answer 21

is this correct

Answer 22

whre as - shows the decrease in the rate of molecules

Answer 23

Where delta A is the number of molecules?

Answer 24

*Change in number of molecules.

Answer 25

yes

Answer 26

is this the right equation?

Answer 27

what is the time in this case?

Answer 28

The rate must be multiplied by the reciprocal of the stoichiometric coefficient to account for what we just discussed. For a chemical equation:\[aA+bB \rightarrow cC+dD\]Where lower case letters are stoichiometric coefficients and capital letters are some chemical species, the following is true:\[Rate_{rxn}=\frac{-1}{a}\frac{\Delta [A]}{\Delta t}=\frac{-1}{b}\frac{\Delta [B]}{\Delta t}=\frac{1}{c}\frac{\Delta [C]}{\Delta t}=\frac{1}{d}\frac{\Delta [D]}{\Delta t}\]Does that make sense? This is basically the equation you gave, except it didn't take into account the stoichiometric coefficients.

Answer 29

I got it . but in this question how will I find the value ?

Answer 30

do I have to add the values of all the reactant and product sides/