Class 9 Exam > Class 9 Questions > 4.48 L of CH₄ at STP is equal toa) 3.2 g of C...
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4.48 L of CH₄ at STP is equal to
a) 3.2 g of CH₄
b) 0.5 mol of CH₄
c) 1.2 x 1023 molecules of CH₄
d) 0.1 mol of CH₄
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2...
To determine the correct answer, we need to understand the concept of STP (Standard Temperature and Pressure) and the relationship between volume, moles, and molecules of a gas.
1. STP (Standard Temperature and Pressure):
STP refers to a set of standard conditions for temperature and pressure used for comparing and analyzing gases. At STP, the temperature is 0 degrees Celsius (273.15 Kelvin) and the pressure is 1 atmosphere (atm).
2. 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 law allows us to establish a relationship between the volume of a gas and the number of molecules present.
3. Relationship between Volume and Moles:
The volume of a gas is directly proportional to the number of moles of the gas when the temperature and pressure are constant. This relationship can be expressed using the ideal gas equation:
PV = nRT
Where:
- P is the pressure
- V is the volume
- n is the number of moles
- R is the ideal gas constant
- T is the temperature in Kelvin
From this equation, we can rearrange it to solve for the number of moles:
n = PV / RT
4. Relationship between Moles and Molecules:
One mole of a substance contains Avogadro's number of particles, which is approximately 6.022 x 10^23. Therefore, the number of molecules can be calculated using the following equation:
Number of molecules = number of moles x Avogadro's number
Now, let's calculate the number of molecules in 4.48 L of CH4 at STP.
Given:
Volume (V) = 4.48 L
Temperature (T) = 0 degrees Celsius = 273.15 K (STP)
Pressure (P) = 1 atm
Molar mass of CH4 = 16.04 g/mol
1. Convert Volume to Moles:
Using the ideal gas equation, we can calculate the number of moles:
n = PV / RT
= (1 atm) * (4.48 L) / (0.0821 L.atm/mol.K * 273.15 K)
≈ 0.202 mol
2. Convert Moles to Molecules:
Now, we can calculate the number of molecules using Avogadro's number:
Number of molecules = number of moles x Avogadro's number
= 0.202 mol x (6.022 x 10^23 molecules/mol)
≈ 1.217 x 10^23 molecules
Therefore, 4.48 L of CH4 at STP is equal to approximately 1.2 x 10^23 molecules of CH4. Hence, the correct answer is option C.
1. STP (Standard Temperature and Pressure):
STP refers to a set of standard conditions for temperature and pressure used for comparing and analyzing gases. At STP, the temperature is 0 degrees Celsius (273.15 Kelvin) and the pressure is 1 atmosphere (atm).
2. 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 law allows us to establish a relationship between the volume of a gas and the number of molecules present.
3. Relationship between Volume and Moles:
The volume of a gas is directly proportional to the number of moles of the gas when the temperature and pressure are constant. This relationship can be expressed using the ideal gas equation:
PV = nRT
Where:
- P is the pressure
- V is the volume
- n is the number of moles
- R is the ideal gas constant
- T is the temperature in Kelvin
From this equation, we can rearrange it to solve for the number of moles:
n = PV / RT
4. Relationship between Moles and Molecules:
One mole of a substance contains Avogadro's number of particles, which is approximately 6.022 x 10^23. Therefore, the number of molecules can be calculated using the following equation:
Number of molecules = number of moles x Avogadro's number
Now, let's calculate the number of molecules in 4.48 L of CH4 at STP.
Given:
Volume (V) = 4.48 L
Temperature (T) = 0 degrees Celsius = 273.15 K (STP)
Pressure (P) = 1 atm
Molar mass of CH4 = 16.04 g/mol
1. Convert Volume to Moles:
Using the ideal gas equation, we can calculate the number of moles:
n = PV / RT
= (1 atm) * (4.48 L) / (0.0821 L.atm/mol.K * 273.15 K)
≈ 0.202 mol
2. Convert Moles to Molecules:
Now, we can calculate the number of molecules using Avogadro's number:
Number of molecules = number of moles x Avogadro's number
= 0.202 mol x (6.022 x 10^23 molecules/mol)
≈ 1.217 x 10^23 molecules
Therefore, 4.48 L of CH4 at STP is equal to approximately 1.2 x 10^23 molecules of CH4. Hence, the correct answer is option C.
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Community Answer
4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2...
Methane (CH4) is a gas and we know for gases at STP,
22.4 L = 1 mole gas
⇒ 4.48 L of methane gas = 4.48/22.4 = 0.2 moles
∵ 1 mole of CH4 = 6.022 x 1023 molecules of methane
∴ 0.2 mole of CH4 = 6.022 x 1023 x 0.2 = 1.2 x 1023 molecules
22.4 L = 1 mole gas
⇒ 4.48 L of methane gas = 4.48/22.4 = 0.2 moles
∵ 1 mole of CH4 = 6.022 x 1023 molecules of methane
∴ 0.2 mole of CH4 = 6.022 x 1023 x 0.2 = 1.2 x 1023 molecules
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4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer?
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4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer? for Class 9 2024 is part of Class 9 preparation. The Question and answers have been prepared according to the Class 9 exam syllabus. Information about 4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 9 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer?.
4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer? for Class 9 2024 is part of Class 9 preparation. The Question and answers have been prepared according to the Class 9 exam syllabus. Information about 4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 9 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer?.
Solutions for 4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 9.
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4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer?, a detailed solution for 4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer? has been provided alongside types of 4.48 L of CH₄ at STP is equal toa) 3.2 g of CH₄b) 0.5 mol of CH₄c) 1.2 x 1023 molecules of CH₄d) 0.1 mol of CH₄Correct answer is option 'C'. Can you explain this answer? theory, EduRev gives you an
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