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Anon25 [30]
3 years ago
14

If the initial concentration of NOBr is 0.0440 M, the concentration of NOBr after 9.0 seconds is ________. If the initial concen

tration of is 0.0440 , the concentration of after 9.0 seconds is ________. 0.0325 M 0.0276 M 0.0403 M 0.0334 M 0.0342 M
Chemistry
1 answer:
Nikolay [14]3 years ago
5 0

This is an incomplete question, here is a complete question.

If the initial concentration of NOBr is 0.0440 M, the concentration of NOBr after 9.0 seconds is ________.

The reaction

2NOBr(g)\rightarrow 2NO(g)+Br_2(g)

It is a second-order reaction with a rate constant of 0.80 M⁻¹s⁻¹ at 11 °C.

Answer : The concentration of after 9.0 seconds is, 0.00734 M

Explanation :

The integrated rate law equation for second order reaction follows:

k=\frac{1}{t}\left (\frac{1}{[A]}-\frac{1}{[A]_o}\right)

where,

k = rate constant = 0.80 M⁻¹s⁻¹

t = time taken  = 142 second

[A] = concentration of substance after time 't' = ?

[A]_o = Initial concentration = 0.0440 M

Putting values in above equation, we get:

0.80M^{-1}s^{-1}=\frac{1}{142s}\left (\frac{1}{[A]}-\frac{1}{(0.0440M)}\right)

[A]=0.00734M

Hence, the concentration of after 9.0 seconds is, 0.00734 M

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For many years chloroform (CHCl3) was used as an inhalation anesthetic in spite of the fact that it is also a toxic substance th
Debora [2.8K]

Hey there!:

Molar mass:

CHCl3 = ( 12.01 * 1 )+ (1.008 * 1 ) + ( 35.45 * 3 ) => 119.37 g/mol

C% =  ( atomic mass C / molar mass CHCl3 ) * 100

For C :

C % =  (12.01 / 119.37 ) * 100

C% = ( 0.1006 * 100 )

C% =  10.06 %

For H :

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H% = ( 1.008 / 119.37 ) * 100

H% = 0.008444 * 100

H% = 0.8444 %

For Cl :

Cl % ( molar mass Cl3 / molar mass CHCl3 ):

Cl% =  ( 3 * 35.45 / 119.37 ) * 100

Cl% =  ( 106.35 / 119.37 ) * 100

Cl% = 0.8909 * 100

Cl% = 89.9%


Hope that helps!

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