3. Nitrogen, when combined with oxygen, can form various oxides. 3.5 g of nitrogen gas is burned in oxygen to form 11.5 g of an oxide of nitrogen. a) Determine the mass of oxygen burned. (Hint: The oxide contains ONLY nitrogen and oxygen!) b)Using the data from the experiment, find the percent of nitrogen by mass in the oxide. c) Using the data from the experiment, find the percent of oxygen by mass in the oxide. d) Use the data from this experiment to find the empirical formula of the oxide of nitrogen. e) If you were given a 100. mg sample of the oxide, how many milligrams of nitrogen would be in your sample?
3. Nitrogen, when combined with oxygen, can form various oxides. 3.5 g of nitrogen gas is burned in oxygen to form 11.5 g of an oxide of nitrogen. a) Determine the mass of oxygen burned. (Hint: The oxide contains ONLY nitrogen and oxygen!) b)Using the data from the experiment, find the percent of nitrogen by mass in the oxide. c) Using the data from the experiment, find the percent of oxygen by mass in the oxide. d) Use the data from this experiment to find the empirical formula of the oxide of nitrogen. e) If you were given a 100. mg sample of the oxide, how many milligrams of nitrogen would be in your sample?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter2: Atoms, Molecules, And Ions
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Problem 90QAP: Calculate the average density of a single Al-27 atom by assuming that it is a sphere with a radius...
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The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
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When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
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1) The question screenshot has been attached down below answer ques 3 d,e step-by-step. I am also putting the screenhot for 3 a,b,c solution for ur reference.
Transcribed Image Text:3) a) Determine the mass of oxygen burned:
The reaction is as follows:
N + XQ -> NOx
According to the law of conservation of mass, the total mass of the reactants is equal to the total mass of
the products. In this reaction,
Mass of N₂ + Mass of O₂ = mass of an oxide of nitro
Hence, the mass of oxygen burned is 8.0g.
b) Find the percent of nitrogen by mass in the oxide:
% nitrogen 3.5g x 100% = 30.43%
11.5g
Hence, the percent of nitrogen by mass in the oxide is 30.43%.
c) Find the percent of oxygen by mass in the oxide:
8.0g
% oxygen = X 100% = 69.57%
11.5g
Hence, the percent of oxygen by mass in the oxide is 69.57%.
Transcribed Image Text:3. Nitrogen, when combined with oxygen, can form various oxides. 3.5 g of nitrogen gas is
burned in oxygen to form 11.5 g of an oxide of nitrogen.
a) Determine the mass of oxygen burned. (Hint: The oxide contains ONLY nitrogen and
oxygen!)
b)Using the data from the experiment, find the percent of nitrogen by mass in the oxide.
c) Using the data from the experiment, find the percent of oxygen by mass in the oxide.
d) Use the data from this experiment to find the empirical formula of the oxide of nitrogen.
e) If you were given a 100. mg sample of the oxide, how many milligrams of nitrogen would
be in your sample?
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