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If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?
(mol wt: N2 = 28, O2 = 32)
- a)Both flasks contain the same number of molecules.
- b)The pressure in the nitrogen flask is greater than the one in the oxygen flask.
- c)More molecules are present in the oxygen flask.
- d)Molecules in the oxygen flask are moving faster on the average than the ones in the nitrogen flask.
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
If equal weights of oxygen and nitrogen are placed in separate contain...
PV = nRT
P = nRT/VP = (mass / mw) RT/V
at the same mass, R, T and V, higher mw --> lower Pressure.. O2 is 32 g/mole.. N2 is 28 g/mole.. O2 is lower pressure than N2
Most Upvoted Answer
If equal weights of oxygen and nitrogen are placed in separate contain...
Explanation:
Statement: If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?
To determine the correct statement, we need to consider the properties of gases and how they relate to the given conditions.
1. Avogadro's Law:
According to Avogadro's law, equal volumes of gases at the same temperature and pressure contain an equal number of molecules. This means that if the containers have the same volume, then they will contain the same number of molecules.
2. Molar Mass:
The molar mass of nitrogen (N2) is 28 g/mol and the molar mass of oxygen (O2) is 32 g/mol.
3. Equal Weights:
The statement mentions that equal weights of oxygen and nitrogen are placed in separate containers. Since the molar masses of nitrogen and oxygen are different, equal weights of these gases will correspond to different numbers of moles.
Analysis:
Given that the weights of oxygen and nitrogen are equal, but their molar masses are different, it means that the number of moles of each gas will be different.
Let's assume that the weight of each gas is 28 grams (since N2 has a molar mass of 28 g/mol). The number of moles of nitrogen can be calculated using the formula:
Number of moles = weight / molar mass
For nitrogen:
Number of moles = 28 g / 28 g/mol = 1 mol
For oxygen:
Number of moles = 28 g / 32 g/mol = 0.875 mol
Conclusion:
From the above calculations, we can conclude that the number of moles of nitrogen is greater than the number of moles of oxygen when equal weights of these gases are considered.
Therefore, the correct statement is:
b) The pressure in the nitrogen flask is greater than the one in the oxygen flask.
Explanation:
The pressure exerted by a gas is directly proportional to the number of moles of the gas. Since the nitrogen flask contains more moles of gas compared to the oxygen flask, the pressure in the nitrogen flask will be greater.
Statement: If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?
To determine the correct statement, we need to consider the properties of gases and how they relate to the given conditions.
1. Avogadro's Law:
According to Avogadro's law, equal volumes of gases at the same temperature and pressure contain an equal number of molecules. This means that if the containers have the same volume, then they will contain the same number of molecules.
2. Molar Mass:
The molar mass of nitrogen (N2) is 28 g/mol and the molar mass of oxygen (O2) is 32 g/mol.
3. Equal Weights:
The statement mentions that equal weights of oxygen and nitrogen are placed in separate containers. Since the molar masses of nitrogen and oxygen are different, equal weights of these gases will correspond to different numbers of moles.
Analysis:
Given that the weights of oxygen and nitrogen are equal, but their molar masses are different, it means that the number of moles of each gas will be different.
Let's assume that the weight of each gas is 28 grams (since N2 has a molar mass of 28 g/mol). The number of moles of nitrogen can be calculated using the formula:
Number of moles = weight / molar mass
For nitrogen:
Number of moles = 28 g / 28 g/mol = 1 mol
For oxygen:
Number of moles = 28 g / 32 g/mol = 0.875 mol
Conclusion:
From the above calculations, we can conclude that the number of moles of nitrogen is greater than the number of moles of oxygen when equal weights of these gases are considered.
Therefore, the correct statement is:
b) The pressure in the nitrogen flask is greater than the one in the oxygen flask.
Explanation:
The pressure exerted by a gas is directly proportional to the number of moles of the gas. Since the nitrogen flask contains more moles of gas compared to the oxygen flask, the pressure in the nitrogen flask will be greater.
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If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?(mol wt: N2 = 28, O2 = 32)a)Both flasks contain the same number of molecules.b)The pressure in the nitrogen flask is greater than the one in the oxygen flask.c)More molecules are present in the oxygen flask.d)Molecules in the oxygen flask are moving faster on the average than the ones in the nitrogen flask.Correct answer is option 'B'. Can you explain this answer?
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If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?(mol wt: N2 = 28, O2 = 32)a)Both flasks contain the same number of molecules.b)The pressure in the nitrogen flask is greater than the one in the oxygen flask.c)More molecules are present in the oxygen flask.d)Molecules in the oxygen flask are moving faster on the average than the ones in the nitrogen flask.Correct answer is option 'B'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?(mol wt: N2 = 28, O2 = 32)a)Both flasks contain the same number of molecules.b)The pressure in the nitrogen flask is greater than the one in the oxygen flask.c)More molecules are present in the oxygen flask.d)Molecules in the oxygen flask are moving faster on the average than the ones in the nitrogen flask.Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?(mol wt: N2 = 28, O2 = 32)a)Both flasks contain the same number of molecules.b)The pressure in the nitrogen flask is greater than the one in the oxygen flask.c)More molecules are present in the oxygen flask.d)Molecules in the oxygen flask are moving faster on the average than the ones in the nitrogen flask.Correct answer is option 'B'. Can you explain this answer?.
If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?(mol wt: N2 = 28, O2 = 32)a)Both flasks contain the same number of molecules.b)The pressure in the nitrogen flask is greater than the one in the oxygen flask.c)More molecules are present in the oxygen flask.d)Molecules in the oxygen flask are moving faster on the average than the ones in the nitrogen flask.Correct answer is option 'B'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?(mol wt: N2 = 28, O2 = 32)a)Both flasks contain the same number of molecules.b)The pressure in the nitrogen flask is greater than the one in the oxygen flask.c)More molecules are present in the oxygen flask.d)Molecules in the oxygen flask are moving faster on the average than the ones in the nitrogen flask.Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?(mol wt: N2 = 28, O2 = 32)a)Both flasks contain the same number of molecules.b)The pressure in the nitrogen flask is greater than the one in the oxygen flask.c)More molecules are present in the oxygen flask.d)Molecules in the oxygen flask are moving faster on the average than the ones in the nitrogen flask.Correct answer is option 'B'. Can you explain this answer?.
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