Answer Happy

Nitrous oxide is used by medical professionals, most famously dentists, to sedate patients. However, too much nitrous oxide can be deadly. Nitrous oxide is part of a reversible reaction as shown below with harmless oxygen and nitrogen gasses. Consider the two scenarios, and suggest what changes could be made to achieve the stated goals by applying concepts from this module. N2 (1+ O2(g) = 2NO(C) AH = 180.7 kJ Scenario 1: A doctor in the emergency department needs to sedate patients quickly. She has a bottle with a mixture of N2, O2, and NO all at equilibrium as shown in the equation above. Suggest a change the hospital could make to this bottle either in storage or short-term use that would help the doctor have more of the substance she needs. Explain why this suggestion would result in the desired outcome. Scenario 2: The risk manager at the hospital is concerned that the bottle might leak when it is in storage and not in use. As part of his training for the job, he took a few chemistry classes. He suggests that the bottle should be stored under more pressure. In the safety meeting he explained, "This would shift the equilibrium in the bottle so that if it does leak, the safer gasses (nitrogen and oxygen) would be released instead of the nitrous oxide." The doctor does not agree with this statement stating that pressure has no effect on the reaction. She believes a different solution should be considered. Evaluate whether the risk manager or the doctor have more appropriate suggestions for this safety concern.