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In the presence of nitric acid, UO 2+ undergoes a redox process. It is converted to UO 2 2+ and nitric oxide (NO) gas is produced according to the following unbalanced equation: H + ( a q ) + NO 3 − ( a q ) + UO 2+ ( a q ) → NO ( g ) + UO 2 2 + ( a q ) + H 2 O ( l ) If 2.55 × 10 2 mL NO( g ) is isolated at 29°C and 1.5 atm, what amount (moles) of UO 2+ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 165IP
Textbook Problem
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In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric oxide (NO) gas is produced according to the following unbalanced equation:

H + ( a q ) +  NO 3 ( a q ) +  UO 2+ ( a q )  NO ( g )   + UO 2 2 + ( a q )   + H 2 O ( l )

If 2.55 × 102 mL NO(g) is isolated at 29°C and 1.5 atm, what amount (moles) of UO2+ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)

Interpretation Introduction

Interpretation: The number of moles of UO2+ used in the given reaction is to be determined if the volume of NO is isolated is 2.55×102mL at 29oC and 1.5atm .

Concept introduction:

  • Balance equation is the chemical equation of a reaction which is written according to law of conservation of mass.
  • Number of moles of a substance, According to ideal gas equation,

Numberofmoles=Pressure×VolumeR×Temperature

  • Mole ratios between the reactant and a product of a reaction are depends upon the coefficients of reactant and product in a balanced chemical equation.

Explanation of Solution

Explanation

To find: the balanced chemical equation of the given unbalanced equation of reaction.

2H++2NO3+3UO2+3UO22++2NO+H2O

The chemical equation of the reaction is given as,

H++NO3+UO2+UO22++NO+H2O

This equation is not balanced, Balanced equation is the chemical equation of a reaction which is written according to law of conservation of mass the mass of reactant molecules should conserve in product molecules.

The balanced chemical equation of the given reaction is,

Balance the molecules in both sides of arrow in order of oxidation states of molecules. Here, each uranium atom loss two electrons and each nitrogen atoms gain three electrons. Therefore to balance these electrons transfer, nitrogen is needed to multiply with two and uranium is needed to multiply with three.

Therefore the balanced chemical equation of the given reaction will be,

2H++2NO3+3UO2+3UO22++2NO+H2O

To find: the number of moles of NO is formed in the given reaction at 29oC and 1.5atm .

The number of moles of NO is 0.015mol .

The volumes of NO is given as 2.55×102mL=0.255L .

The pressure of NO is given as 1.5atm .

The temperature is 29oC=(29+273)K=302K .

The equation for finding number of moles of a substance, According to ideal gas equation,

Numberofmoles=Pressure×VolumeR×Temperature

Therefore,

The number of moles of NO in the given reaction is,

nNO=1

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Chemistry: An Atoms First Approach
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