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Soloha48 [4]
3 years ago
15

When a mixture of oxygen and hydrogen is ignited in a test tube, the

Chemistry
1 answer:
KiRa [710]3 years ago
8 0

Answer:

follow me and pm and I answer your question

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The rate constant, k, for a reaction is 0.0354 sec1 at 40°C. Calculate the rate constant for the
deff fn [24]

Answer:

The rate constant of the reaction at 125˚ is 0.3115 \ \text{sec}^{-1}.

Explanation:

The Arrhenius equation is a simple equation that describes the dependent relationship between temperature and the rate constant of a chemical reaction. The Arrhenius equation is written mathematically as

                                                  k \ = \ Ae^{\displaystyle\frac{-E_{a}}{RT}}

                                               \ln k \ = \ \ln A \ - \ \displaystyle\frac{E_{a}}{RT}

where k is the rate constant, E_{a} represents the activation energy of the chemical reaction, R is the gas constant, T is the temperature, and A is the frequency factor.

The frequency factor, A, is a constant that is derived experimentally and numerically that describes the frequency of molecular collisions and their orientation which varies slightly with temperature but this can be assumed to be constant across a small range of temperatures.

Consider that the rate constant be k_{1} at an initial temperature T_{1} and the rate constant k_{2} at a final temperature T_{2}, thus

                         \ln k_{2} \ - \ \ln k_{1} = \ \ln A \ - \ \displaystyle\frac{E_{a}}{RT_{2}} \ - \ \left(\ln A \ - \ \displaystyle\frac{E_{a}}{RT_{1}}\right) \\ \\ \\ \rule{0.62cm}{0cm} \ln \left(\displaystyle\frac{k_{2}}{k_{1}}\right) \ = \ \displaystyle\frac{E_{a}}{R}\left(\displaystyle\frac{1}{T_{1}} \ - \ \displaystyle\frac{1}{T_{2}} \right)

                                         \rule{1.62cm}{0cm} \displaystyle\frac{k_{2}}{k_{1}} \ = \ e^{\displaystyle\frac{E_{a}}{R}\left(\displaystyle\frac{1}{T_{1}} \ - \ \displaystyle\frac{1}{T_{2}} \right)} \\ \\ \\ \rule{1.62cm}{0cm} k_{2} \ = \ k_{1}e^{\displaystyle\frac{E_{a}}{R}\left(\displaystyle\frac{1}{T_{1}} \ - \ \displaystyle\frac{1}{T_{2}} \right)}

Given that E_{a} \ = \ 26.5 \ \ \text{kJ/mol}, R \ = \ 8.3145 \ \ \text{J mol}^{-1} \ \text{K}^{-1}, T_{1} \ = \ \left(40 \ + \ 273\right) \ K, T_{2} \ = \ \left(125 \ + \ 273\right) \ K, and k_{1} \ = \ 0.0354 \ \ \text{sec}^{-1}, therefore,

           k_{2} \ = \ \left(0.0354 \ \ \text{sec}^{-1}\right)e^{\displaystyle\frac{26500 \ \text{J mol}^{-1}}{8.3145 \ \text{J mol}^{-1} \ \text{K}^{-1}}\left(\displaystyle\frac{1}{313 \ \text{K}} \ - \ \displaystyle\frac{1}{398 \ \text{K}} \right)} \\ \\ \\ k_{2} \ = \ 0.3115 \ \ \text{sec}^{-1}                      

8 0
2 years ago
What mass of KCl is contained in 3.00 L of solution that has a molarity of 1.50M
Soloha48 [4]

Answer:

335.25g

Explanation:

using equation of molarity

8 0
3 years ago
Read 2 more answers
What is the density (g/mL) of an object that has a mass of 0.03 kg and occupies a volume of 25 mL?
tatyana61 [14]
First convert the kg to g ----- 0.03kg = 30g
Then divide the mass by the volume ----- 30g ÷ 25mL = 1.2
The density is 1.2g/mL<span />
5 0
3 years ago
Read 2 more answers
Test questions Accidently did this
PSYCHO15rus [73]
I don’t see any questions
6 0
3 years ago
Read 2 more answers
How carbon dioxide prepared in lab?
Nana76 [90]

Explanation:

In laboratory, carbon dioxide is not obtained from the air, carbon dioxide is prepared from carbonates by adding acids to the carbonates. In this experiment carbon dioxide is prepared by the reaction of marble with hydrochloric acid.

7 0
3 years ago
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