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Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)
In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.
[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]
In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.
[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]
Correct answer is between '4.8,5.0'. Can you explain this answer?
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Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l...
Calculation of moles of Cu used:
- Given mass of Cu = 6.36 g
- Atomic mass of Cu = 63.6 g/mol
- Moles of Cu used = 6.36 g / 63.6 g/mol = 0.1 mol
Calculation of moles of NO2 produced:
- From the balanced chemical equation, 2 moles of NO2 are produced for every 1 mole of Cu used.
- Therefore, moles of NO2 produced = 2 x 0.1 mol = 0.2 mol
Calculation of volume of NO2 produced:
- Ideal gas law equation: PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, and T is temperature.
- Rearranging the equation: V = (nRT)/P
- Given pressure (P) = 1 atm, temperature (T) = 298 K, gas constant (R) = 0.0821 L atm K^-1 mol^-1, and moles of NO2 produced (n) = 0.2 mol
- Substituting the values: V = (0.2 mol x 0.0821 L atm K^-1 mol^-1 x 298 K) / 1 atm = 4.97 L
- Rounding off to one decimal place: 4.97 L ≈ 5.0 L
Therefore, the volume of NO2 produced in liters is approximately 5.0 L.
- Given mass of Cu = 6.36 g
- Atomic mass of Cu = 63.6 g/mol
- Moles of Cu used = 6.36 g / 63.6 g/mol = 0.1 mol
Calculation of moles of NO2 produced:
- From the balanced chemical equation, 2 moles of NO2 are produced for every 1 mole of Cu used.
- Therefore, moles of NO2 produced = 2 x 0.1 mol = 0.2 mol
Calculation of volume of NO2 produced:
- Ideal gas law equation: PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, and T is temperature.
- Rearranging the equation: V = (nRT)/P
- Given pressure (P) = 1 atm, temperature (T) = 298 K, gas constant (R) = 0.0821 L atm K^-1 mol^-1, and moles of NO2 produced (n) = 0.2 mol
- Substituting the values: V = (0.2 mol x 0.0821 L atm K^-1 mol^-1 x 298 K) / 1 atm = 4.97 L
- Rounding off to one decimal place: 4.97 L ≈ 5.0 L
Therefore, the volume of NO2 produced in liters is approximately 5.0 L.
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Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]Correct answer is between '4.8,5.0'. Can you explain this answer?
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Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]Correct answer is between '4.8,5.0'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]Correct answer is between '4.8,5.0'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]Correct answer is between '4.8,5.0'. Can you explain this answer?.
Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]Correct answer is between '4.8,5.0'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]Correct answer is between '4.8,5.0'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]Correct answer is between '4.8,5.0'. Can you explain this answer?.
Solutions for Cu(s) + 4 H+(aq) + 2NO3–(aq) → 2NO2(g) + Cu2+(aq) + 2H2O(l)In the above reaction at 1 atm and 298 K, if 6.36 g of copper is used. Assuming ideal gas behavior, the volume of NO2 produced in liters is __.[Given: atomic mass of Cu is 63.6; R = 0.0821 L atm K–1 mol–1]Correct answer is between '4.8,5.0'. Can you explain this answer? in English & in Hindi are available as part of our courses for Chemistry.
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