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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
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.

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) 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%.
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?
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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