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umka2103 [35]
3 years ago
10

A certain first-order reaction has a rate constant of 2.15×10−2 s−1 at 20 ∘C. What is the value of k at 55 ∘C if Ea = 72.0 kJ/mo

l ?
Chemistry
1 answer:
adell [148]3 years ago
3 0

Answer:

k_2=0.504s^{-1}

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to calculate the rate constant at 55 °C by using the temperature-variable version of the Arrhenius equation:

ln(\frac{k_2}{k_1} )=-\frac{Ea}{R}(\frac{1}{T_2} -\frac{1}{T_1} )

Thus, we plug in the temperatures, activation energy and universal constant of gases in consistent units to obtain:

ln(\frac{k_2}{0.0215s^{-1}} )=-\frac{72000\frac{J}{mol}}{8.3145\frac{J}{mol*K}}(\frac{1}{55+273} -\frac{1}{20+273} ) \\\\ln(\frac{k_2}{0.0215s^{-1}} )=3.154\\\\k_2=0.0215s^{-1}exp(3.154)\\\\k_2=0.504s^{-1}

Regards!

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Explanation:

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1. Starting with 9.3 moles of O 2 , how many moles of H 2 S will be needed and how many moles of SO 2 will
enyata [817]

Answer:

Moles of H₂S needed = 6.2 mol

Moles of SO₂ produced = 6.2 mol

Explanation:

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Number of moles of O₂ = 9.3 mol

Moles of H₂S needed = ?

Moles of SO₂ produced = ?

Solution:

Chemical equation:

2H₂S + 3O₂      →    2SO₂ + 2H₂O

Now we will compare the moles of oxygen with H₂S.

                  O₂             :           H₂S

                    3             :             2

                   9.3            :         2/3×9.3 = 6.2 mol

Now we will compare the moles of SO₂ with both reactant.

                   O₂             :            SO₂

                    3              :               2

                   9.3            :         2/3×9.3 = 6.2 mol      

                 H₂S             :            SO₂

                    2              :               2

                   6.2            :          6.2 mol      

So 6.2 moles of  SO₂ are produced.

         

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