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Annette [7]
3 years ago
8

The reactant concentration in a second-order reaction was 0.560 m after 115 s and 3.30×10−2 m after 735 s . what is the rate con

stant for this reaction?
Chemistry
1 answer:
Aloiza [94]3 years ago
3 0
Use the formula for second order reaction:

\frac{1}{C} = \frac{1}{C_0} + kt

C = concentration at time t 
C0 =  initial conc.
k = rate constant
t = time

1st equation :   \frac{1}{0.56} = \frac{1}{C_0} + 115k

2nd Equation: \frac{1}{0.033} = \frac{1}{C_0} + 735k

Find \frac{1}{C_0} from 1st equation and put it in 2nd equation:

\frac{1}{0.033} = \frac{1}{0.56} - 115k + 735k

\frac{1}{0.033} - \frac{1}{0.56} = 620k

k = 0.046
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2 years ago
Explain why the electron configuration of 2-3-1 represents an atom in an excited state?
baherus [9]

Answer:

See explanation

Explanation:

If we look at the electron configuration closely, we will discover that the element must have had a ground state electron configuration of 2,4.

This is because, the innermost shell usually holds two electrons while the outer shells hold eight electrons each. The four electrons must be accommodated in the second shell in the ground state configuration of the compound.

However, when the atom is excited, one electron from this shell may move to the third shell to give the excited state configuration 2-3-1 as shown in the question.

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2 years ago
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klemol [59]

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5 0
8 months ago
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O 3 ( g ) + NO ( g )
Aleksandr [31]

Answer:

(a) 7.11x10⁻⁴ M/s

(b) 2.56 mol.L⁻¹.h⁻¹

Explanation:

(a) The reaction is:

O₃(g) + NO(g) → O₂(g) + NO₂(g)   (1)

The reaction rate of equation (1) is given by:

rate = k*[O_{3}][NO]     (2)

<u>We have:</u>

k: is the rate constant of reaction = 3.91x10⁶ M⁻¹.s⁻¹

[O₃]₀ = 2.35x10⁻⁶ M

[NO]₀ = 7.74x10⁻⁵ M

Hence, to find the inital reacion rate we will use equation (2):

rate = k*[O_{3}]_{0}[NO]_{0} = 3.91 \cdot 10^{6} M^{-1}s^{-1}*2.35\cdot 10^{-6} M*7.74 \cdot 10^{-5} M = 7.11 \cdot 10^{-4} M/s  

Therefore, the inital reaction rate is 7.11x10⁻⁴ M/s

(b) The number of moles of NO₂(g) produced per hour per liter of air is:

t = 1 h

V = 1 L

\frac{\Delta[NO_{2}]}{\Delta t} = rate

\frac{\Delta[NO_{2}]}{\Delta t} = 7.11 \cdot 10^{-4} M/s*\frac{3600 s}{1 h} = 2.56 mol.L^{-1}.h{-1}

Hence, the number of moles of NO₂(g) produced per hour per liter of air is 2.56 mol.L⁻¹.h⁻¹

I hope it helps you!                                

5 0
2 years ago
C. Why do chemists routinely test existing chemicals?
frozen [14]

Answer :

The chemists such as analytical chemists determine the structure, composition, and nature of substances by examining and identifying their various elements or compounds. These chemists are crucial to the pharmaceutical industry because pharmaceutical companies need to know the identity of compounds that they hope to turn into drugs.

8 0
2 years ago
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