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zloy xaker [14]
2 years ago
7

Nitrogen dioxide is used industrially to produce nitric acid, but it contributes to acid rain and photochemical smog. What volum

e (in L) of nitrogen dioxide is formed at 735 torr and 28.2°C by reacting 4.95 cm³ of copper (d = 8.95 g/cm³) with 230.0 mL of nitric acid (d 5 1.42 g/cm³, 68.0% HNO₃ by mass)? Cu(s) + 4HNO₃(aq) → Cu(NO₃)₂(aq) + 2NO₂(g) + 2H₂O(l)
Chemistry
1 answer:
Gnom [1K]2 years ago
4 0

The reaction of nitric acid with copper is:

Cu(s) + 4HNO₃ → Cu(NO₃)₂ + 2NO₂(g) + 2H₂O(l)

Moles of copper are: 4.95cm3 X8.95gmX1mol  / 63.55gmX1mol

=0.697moles

Moles of nitric acid are: 230mlX 1.42gm X68gmX1mol / 63.01gmX100gm

=3.52moles

As 1 mol of Cu reacts with 4 moles of HNO₃  

=0.697 mol Cu × (4mol HNO₃ / 1mol Cu) = 2.79 moles of HNO₃ will react. That means Cu is limiting reactant.

Moles of NO₂ produced are:

0.697 mol Cu × (2mol NO₂ / 1mol Cu) = 1.394 moles of NO₂

Using PV = nRT

Where P is pressure (735torr / 760 = 0.967atm) ; n are moles (1.394mol);

R is gas constant (0.082atmL/molK); T is temperature (28.2°C + 273.15 = 301.35K).

Thus, volume is:V = nRT / P

V = 1.394mol×0.082atmL/molK×301.35K / 0.967atm

V = 35.6L

The volume of nitrogen oxide formed is 35.6L

To know more about nitrogen dioxide  here

brainly.com/question/15682963

#SPJ4

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