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3b. An impure sample of ammonium dichromate [ (NH4)2Cr207] was analyzed to determine its purity [ %(m/m) of ammonium dichromate]. a. A 1.4325 gram sample of the impure (NH4)2C12O7 was heated and decomposed in the following (unbalanced equation) reaction: • Balance the chemical equation: [ Select ] (NH4)2C12O7(s) [ Select ] N2(g) + [ [ Select ] H2O(L) + [ Select ] Cr203(s) b. The decomposition of the 1.4325 g of the impure sample produces 0.1252 liters of nitrogen gas (N2(9)) that were collected at a temperature of 24.7°C and a pressure of 1.032 atmospheres: • Calculate the number of moles of nitrogen (N2(g)) collected in this reaction: [ Select ] mol N2 • Calculate the mass of the ammonium dichromate [ (NH4)2Cr207 ] in the sample (1.4325 g): [ Select ] g (NH4)2Cr207 • Calculate the %(m/m) of the ammonium dichromate in the impure sample: [ Select ] | %(m/m) (NH4)¿Cr207

3b. An impure sample of ammonium dichromate [ (NH4)2Cr207] was analyzed to determine its purity [ %(m/m) of ammonium dichromate]. a. A 1.4325 gram sample of the impure (NH4)2C12O7 was heated and decomposed in the following (unbalanced equation) reaction: • Balance the chemical equation: [ Select ] (NH4)2C12O7(s) [ Select ] N2(g) + [ [ Select ] H2O(L) + [ Select ] Cr203(s) b. The decomposition of the 1.4325 g of the impure sample produces 0.1252 liters of nitrogen gas (N2(9)) that were collected at a temperature of 24.7°C and a pressure of 1.032 atmospheres: • Calculate the number of moles of nitrogen (N2(g)) collected in this reaction: [ Select ] mol N2 • Calculate the mass of the ammonium dichromate [ (NH4)2Cr207 ] in the sample (1.4325 g): [ Select ] g (NH4)2Cr207 • Calculate the %(m/m) of the ammonium dichromate in the impure sample: [ Select ] | %(m/m) (NH4)¿Cr207

Chemistry
Chemistry
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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
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3b. An impure sample of ammonium dichromate [ (NH4)2Cr207] was analyzed to determine its purity [ %(m/m) of ammonium dichromate]. a. A 1.4325 gram sample of the impure (NH4)2Cr207 was heated and decomposed in the following (unbalanced equation) reaction: • Balance the chemical equation: [ Select ] (NH4)2Cr2O7(s) [ Select ] N2(g) [ Select ] H20(L) + + [ Select ] | Cr2O3(s) b. The decomposition of the 1.4325 g of the impure sample produces 0.1252 liters of nitrogen gas (N2(g) that were collected at a temperature of 24.7°C and a pressure of 1.032 atmospheres: o Calculate the number of moles of nitrogen (N2(g)) collected in this reaction: [ Select ] mol N2 • Calculate the mass of the ammonium dichromate [ (NH4)2Cr20, ] in the sample (1.4325 g): [ Select ] g (NH4)2Cr2O7 o Calculate the %(m/m) of the ammonium dichromate in the impure sample: [ Select ] %(m/m) (NH4)2Cr2O7
Transcribed Image Text:3b. An impure sample of ammonium dichromate [ (NH4)2Cr207] was analyzed to determine its purity [ %(m/m) of ammonium dichromate]. a. A 1.4325 gram sample of the impure (NH4)2Cr207 was heated and decomposed in the following (unbalanced equation) reaction: • Balance the chemical equation: [ Select ] (NH4)2Cr2O7(s) [ Select ] N2(g) [ Select ] H20(L) + + [ Select ] | Cr2O3(s) b. The decomposition of the 1.4325 g of the impure sample produces 0.1252 liters of nitrogen gas (N2(g) that were collected at a temperature of 24.7°C and a pressure of 1.032 atmospheres: o Calculate the number of moles of nitrogen (N2(g)) collected in this reaction: [ Select ] mol N2 • Calculate the mass of the ammonium dichromate [ (NH4)2Cr20, ] in the sample (1.4325 g): [ Select ] g (NH4)2Cr2O7 o Calculate the %(m/m) of the ammonium dichromate in the impure sample: [ Select ] %(m/m) (NH4)2Cr2O7
Expert Solution
Step 1

Given, 

The mass of an impure (NH4)2Cr2O7 is 1.4325g.

The balanced equation is:

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