1. In a hypothetical reaction leading to the formation of carbon dioxide, it was

Question

1. In a hypothetical reaction leading to the formation of carbon dioxide, it was found that at 237 seconds the concentration of carbon dioxide was 0.333 mol/L and at 691.7 seconds the concentration of carbon dioxide was 0.838 mol/L. What is the rate of formation of carbon dioxide over the specified time period in this reaction? Enter your answer to two decimal places.

2.n a certain decomposition reaction, dinitrogen pentoxide decomposes to form nitrogen dioxide gas and oxygen gas. It was found that at 260 seconds the concentration of oxygen gas was 0.25 mol/L and at 683 seconds the concentration of oxygen gas was 0.626 mol/L. What is the rate of decomposition of dinitrogen pentoxide over the specified time period in this reaction? Enter your answer to two decimal places.

3.The reaction for the decomposition of dinitrogen pentoxide to form nitrogen dioxide and oxygen gas has the rate constant 1.7 x 10-3 s-1. This is a first order reaction. How long would it take for for the reaction to be 49.00% to complete? Enter your answer to 1 decimal place even if that is more sig figs that you are entitled to report.

Explanation / Answer

1)
rate = delta concentration / delta time
rate = (0.663 - 0.235) mole/liter / (632.2 - 295) sec = ?? mole/liter/sec

2)

The rates of formation of products and consumption of reactants follows the stoichiometry of the reaction. First, balance the reaction:
2 N2O5 (g) ? 4 NO2 (g) + O2 (g)
This means the NO2 will be produced at 4 times the rate that O2 is produced, and N2O5 will be consumed at twice the rate that O2 is produced. The rate of production of O2 is:
?[O2]/?t = (0.983 mol/L - 0.243 mol/L) / (605.1 s - 381 s) = 0.0033 mol/L

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