--CH3NH2(g)+---02(g)= CO2(g)+----H2O(g)+----N2(g) Consider the oxidation of methylamine shown in the image above. a.When properly balanced the coefficient infront of O2= ? b. If you want to combust 45.0 g of CH3NH2, how many grams of O2 do you need? c. How many grams of N2 gas can be formed from this oxidation?
--CH3NH2(g)+---02(g)= CO2(g)+----H2O(g)+----N2(g) Consider the oxidation of methylamine shown in the image above. a.When properly balanced the coefficient infront of O2= ? b. If you want to combust 45.0 g of CH3NH2, how many grams of O2 do you need? c. How many grams of N2 gas can be formed from this oxidation?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 5PS: Oxidation of 1.00 g of carbon monoxide, CO, produces 1.57 g of carbon dioxide, CO2. How many grams...
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---CH3NH2(g)+---02(g)= CO2(g)+----H2O(g)+----N2(g)
Consider the oxidation of methylamine shown in the image above.
a.When properly balanced the coefficient infront of O2= ?
b. If you want to combust 45.0 g of CH3NH2, how many grams of O2 do you need?
c. How many grams of N2 gas can be formed from this oxidation?
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