Problem: What volume of O2 at STP is required to oxidize 8.0 L of NO at STP to NO2? What volume of NO2 is produced at STP?

🤓 Based on our data, we think this question is relevant for Professor Jackson's class at KU.

FREE Expert Solution

First thing is to write the equation of NO reacting with O2 producing NO2

NO (g) + O(g) → NO2 (g)

Balance O first then N, balanced reaction is:

2NO (g) + O(g) → 2NO2 (g)

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Problem Details

What volume of O2 at STP is required to oxidize 8.0 L of NO at STP to NO2? What volume of NO2 is produced at STP?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Standard Temperature and Pressure concept. You can view video lessons to learn Standard Temperature and Pressure. Or if you need more Standard Temperature and Pressure practice, you can also practice Standard Temperature and Pressure practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Jackson's class at KU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.