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pashok25 [27]
3 years ago
13

Please include an explanation

Chemistry
1 answer:
Vesna [10]3 years ago
4 0

Answer:

The explanation to your question is below.

Explanation:

In thermochemistry, reactions are classify in two groups.

- Endothermic reactions: are reactions that need energy (heat) from the surroundings to happen. If they are not heated, the products will not form.

Example:

                        2 H₂O + energy ⇒ 2H₂  + O₂

-Exothermic reactions: are reactions that release energy to the surroundings. They happen spontaneously.

Example:

                       CH₄  + 2O₂   ⇒   CO₂   +  2H₂O + energy (heat)

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Consider the following reaction 2 N2O(g) =&gt; 2 N2(g) + O2(g) rate = k[N2O]. For an initial concentration of N2O of 0.50 M, cal
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Answer:

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Explanation:

Step 1: Data given

rate = k[N2O]

initial concentration of N2O of 0.50 M

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Step 2: The balanced equation

2N2O(g) → 2 N2(g) + O2(g)  

Step 3: Calculate the concentration of N2O after 2.0 minutes

We use the rate law to derive a time dependent equation.

-d[N2O]/dt = k[N2O]

ln[N2O] = -kt + ln[N2O]i

 ⇒ with k = 3.4 *10^-3 /s

⇒ with t = 2.0 minutes = 120s

⇒ with [N2O]i = initial conc of N2O = 0.50 M

ln[N2O] = -(3.4*10^-3/s)*(120s) + ln(0.5)

ln[N2O] = -1.101

e^(ln[N2O]) = e^(-1.1011)

[N2O} = 0.3325 M

After 2.0 minutes the concentration of N2O is 0.3325 M

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