For the reaction shown, calculate how many moles of NO2 form when each amount of reactant completely reacts.
2 N2O5(g) → 4 NO2(g) + O2(g)
(a) 1.3 mol N2O5
(b) 5.8 mol N2O5
(c) 4.45 × 103 mol N2O5
(d) 1.006 × 10−3 mol N2O5
Here, we are going to calculate the number of moles of NO2 formed when the given amounts of N2O5 completely reacts.
The given chemical reaction is:
2N2O5(g) → 4NO2(g) + O2(g)
From the above equation, it is clear that, 2 moles of N2O5 reacts completely to give 4 moles of NO2 as product.
Therefore, 1 mole of N2O5 will give (4/2 = 2) mol of NO2 on complete reaction.
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The full step-by-step solution to problem: 17P from chapter: 8 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. This full solution covers the following key subjects: mol, Moles, completely, form, amount. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Since the solution to 17P from 8 chapter was answered, more than 2154 students have viewed the full step-by-step answer. The answer to “For the reaction shown, calculate how many moles of NO2 form when each amount of reactant completely reacts.2 N2O5(g) ? 4 NO2(g) + O2(g)(a) 1.3 mol N2O5(b) 5.8 mol N2O5(c) 4.45 × 103 mol N2O5(d) 1.006 × 10?3 mol N2O5” is broken down into a number of easy to follow steps, and 40 words. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295.