SUMMARY
The reaction rate of nitrogen monoxide (NO) and oxygen (O2) to form nitrogen dioxide (NO2) is expressed as r = k [NO]² [O2], where k is the temperature-dependent reaction rate coefficient. When the concentration of NO is doubled and the concentration of O2 is tripled, the reaction rate increases by a factor of 12, calculated as r = k [2*NO]² * [3*O2]. This conclusion is derived from applying the rate law correctly, emphasizing the importance of understanding the impact of concentration changes on reaction rates.
PREREQUISITES
- Understanding of chemical reaction rates and rate laws
- Familiarity with the concepts of concentration and stoichiometry
- Knowledge of the relationship between temperature and reaction rate coefficients
- Basic algebra for manipulating equations
NEXT STEPS
- Study the Arrhenius equation to understand how temperature affects reaction rates
- Learn about reaction mechanisms and their influence on rate laws
- Explore the concept of reaction order and its calculation
- Investigate the effects of catalysts on reaction rates
USEFUL FOR
Chemistry students, educators, and professionals involved in chemical engineering or reaction kinetics who seek to deepen their understanding of reaction rate dynamics.