Azomethane decomposes into nitrogen and ethane at elevated temperature: H3C–N=N–CH3 → N2 + C2H6 A chemist...

Azomethane decomposes into nitrogen and ethane at elevated temperature:
H₃C–N=N–CH₃ → N₂ + C₂H₆
A chemist studying this reaction at 300°C begins an experiment with an azomethane concentration of 8.16 mM and obtains the following data:

Time(s)		100	150	200	250	300
[Azomethane] (mM)		6.32	5.57	4.90	4.31	3.80

Calculate the rate constant. Give an answer with concentration units of molarity and time units of seconds.

Expert Solution

queen_honey_blossom answered 2 years ago

Ethane (C2H6) can rotate around the central C--C bond. When the two -CH3 groups are aligned...

Ethane (C2H6) can rotate around the central C--C bond. When the two -CH3 groups are aligned with each other there is a repulsion between the Hydrogen atoms that results in an energy 2.0 × 10-20 Joules higher than when the Hydrogens are staggered. If the ethane molecules are at room temperature (25° C), what is the ratio of molecules that are perfectly aligned to molecules that are perfectly staggered?

At elevated temperatures, nitrous oxide decomposes according to the equation 2 N2O(g) → 2 N2(g) +...

At elevated temperatures, nitrous oxide decomposes according to the equation 2 N2O(g) → 2 N2(g) + O2(g) Given the following data, plot the appropriate graphs to determine whether the reaction is zeroth, first, or second order. Write the rate equation for this reaction. What is the value of the rate constant for the consumption of N2O? (Use excel to work this problem out completely, show all three graphs and the equations associated with each.) Time (min) 0 60 90 120...

Problem 1. Calculate the average speed of nitrogen molecules (N2) in air at room temperature (∼...

Problem 1. Calculate the average speed of nitrogen molecules (N2) in air at room temperature (∼ 300 K). Compare to the speed of sound, which is about 343 m/s at the same temperature. Speculate on why they might be similar.

A chemist fills a reaction vessel with 1.54 atm nitrogen N 2 gas, 4.42 atm oxygen...

A chemist fills a reaction vessel with 1.54 atm nitrogen N 2 gas, 4.42 atm oxygen O 2 gas, and 8.99 atm nitrogen monoxide NO gas at a temperature of 25.0 ° C . Under these conditions, calculate the reaction free energy Δ G for the following chemical reaction: + N 2 g O 2 g 2 NO g Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. kJ

Question