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How many moles are present in the 1.2dm³ volume of sulphur dioxide gases at r.t.p.?
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+ Inorganic chemistry
+ Chemistry
+ Carbon dioxide
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Julia H.
How many moles are present in the 1.2dm³ volume of sulphur dioxide gases at r.t.p.?
Here’s how you solve this. First, understand that the author is questioning 3 or 4 different concepts, to see if you know them.
[1] MOLES
[2] dm³
[3] SO₂ gas
[4] RTP or STP
Moles are the unit of particles that one atomic mass worth of a homogeneous substance has. An atomic mass is the number of grams of a substance, in grams, that matches its measured or derived atomic mass. . Kind of circular, but that is what it is.
dm³ is cubic decimeters; a decimeter is ¹⁄₁₀ of a meter, so a cubic decimeter is (¹⁄₁₀)³ or ¹⁄₁₀₀₀ of a cubic meter. This, in turn, is the definition of a liter, it being ¹⁄₁₀₀₀ of a cubic meter. Yay! So, the author is asking about liters … and by good fortune, these are the common unit of gas measurements.
SO₂ is sulfur dioxide, a horrid smelling gas, commonly produced by simply burning yellow sulfur in the presence of excess air. As such, it is a gas. So, what do we know about gasses, and moles?
RTP or STP (standard temperature and pressure) is a combination of temperature (273 kelvin or 0 celsius), pressure (1.000 atmosphere, or ‘standard’ sea level), where by one can say with well tested authority that 22.41 liters of a gas, at 273 kelvin and 1.00000 atmosphere … contains exactly 1 mole of whatever gas is being discussed or measured.
Well … then that redefines the problem.
STP is given, so there’s no need to convert other temperatures and pressures to it. The number of liters is given (1.20 liters), so dividing by 22.41 then turns that into standard moles. And the sulfur dioxide business has nothing at all to do with the problem, since ‘it is a gas’, and so more-or-less follows the ideal gas laws.
So … you can do that last part yourself. 1.20 divided by 22.41
Here’s how you solve this. First, understand that the author is questioning 3 or 4 different concepts, to see if you know them.
[1] MOLES
[2] dm³
[3] SO₂ gas
[4] RTP or STP
Moles are the unit of particles that one atomic mass worth of a homogeneous substance has. An atomic mass is the number of grams of a substance, in grams, that matches its measured or derived atomic mass. . Kind of circular, but that is what it is.
dm³ is cubic decimeters; a decimeter is ¹⁄₁₀ of a meter, so a cubic decimeter is (¹⁄₁₀)³ or ¹⁄₁₀₀₀ of a cubic meter. This, in turn, is the definition of a liter, it being ¹⁄₁₀₀₀ of a cubic meter. Yay! So, the author is asking about liters … and by good fortune, these are the common unit of gas measurements.
SO₂ is sulfur dioxide, a horrid smelling gas, commonly produced by simply burning yellow sulfur in the presence of excess air. As such, it is a gas. So, what do we know about gasses, and moles?
RTP or STP (standard temperature and pressure) is a combination of temperature (273 kelvin or 0 celsius), pressure (1.000 atmosphere, or ‘standard’ sea level), where by one can say with well tested authority that 22.41 liters of a gas, at 273 kelvin and 1.00000 atmosphere … contains exactly 1 mole of whatever gas is being discussed or measured.
Well … then that redefines the problem.
STP is given, so there’s no need to convert other temperatures and pressures to it. The number of liters is given (1.20 liters), so dividing by 22.41 then turns that into standard moles. And the sulfur dioxide business has nothing at all to do with the problem, since ‘it is a gas’, and so more-or-less follows the ideal gas laws.
So … you can do that last part yourself. 1.20 divided by 22.41
Here’s how you solve this. First, understand that the author is questioning 3 or 4 different concepts, to see if you know them.
[1] MOLES
[2] dm³
[3] SO₂ gas
[4] RTP or STP
Moles are the unit of particles that one atomic mass worth of a homogeneous substance has. An atomic mass is the number of grams of a substance, in grams, that matches its measured or derived atomic mass. . Kind of circular, but that is what it is.
dm³ is cubic decimeters; a decimeter is ¹⁄₁₀ of a meter, so a cubic decimeter is (¹⁄₁₀)³ or ¹⁄₁₀₀₀ of a cubic meter. This, in turn, is the definition of a liter, it being ¹⁄₁₀₀₀ of a cubic meter. Yay! So, the author is asking about liters … and by good fortune, these are the common unit of gas measurements.
SO₂ is sulfur dioxide, a horrid smelling gas, commonly produced by simply burning yellow sulfur in the presence of excess air. As such, it is a gas. So, what do we know about gasses, and moles?
RTP or STP (standard temperature and pressure) is a combination of temperature (273 kelvin or 0 celsius), pressure (1.000 atmosphere, or ‘standard’ sea level), where by one can say with well tested authority that 22.41 liters of a gas, at 273 kelvin and 1.00000 atmosphere … contains exactly 1 mole of whatever gas is being discussed or measured.
Well … then that redefines the problem.
STP is given, so there’s no need to convert other temperatures and pressures to it. The number of liters is given (1.20 liters), so dividing by 22.41 then turns that into standard moles. And the sulfur dioxide business has nothing at all to do with the problem, since ‘it is a gas’, and so more-or-less follows the ideal gas laws.
So … you can do that last part yourself. 1.20 divided by 22.41
Here’s how you solve this. First, understand that the author is questioning 3 or 4 different concepts, to see if you know them.
[1] MOLES
[2] dm³
[3] SO₂ gas
[4] RTP or STP
Moles are the unit of particles that one atomic mass worth of a homogeneous substance has. An atomic mass is the number of grams of a substance, in grams, that matches its measured or derived atomic mass. . Kind of circular, but that is what it is.
dm³ is cubic decimeters; a decimeter is ¹⁄₁₀ of a meter, so a cubic decimeter is (¹⁄₁₀)³ or ¹⁄₁₀₀₀ of a cubic meter. This, in turn, is the definition of a liter, it being ¹⁄₁₀₀₀ of a cubic meter. Yay! So, the author is asking about liters … and by good fortune, these are the common unit of gas measurements.
SO₂ is sulfur dioxide, a horrid smelling gas, commonly produced by simply burning yellow sulfur in the presence of excess air. As such, it is a gas. So, what do we know about gasses, and moles?
RTP or STP (standard temperature and pressure) is a combination of temperature (273 kelvin or 0 celsius), pressure (1.000 atmosphere, or ‘standard’ sea level), where by one can say with well tested authority that 22.41 liters of a gas, at 273 kelvin and 1.00000 atmosphere … contains exactly 1 mole of whatever gas is being discussed or measured.
Well … then that redefines the problem.
STP is given, so there’s no need to convert other temperatures and pressures to it. The number of liters is given (1.20 liters), so dividing by 22.41 then turns that into standard moles. And the sulfur dioxide business has nothing at all to do with the problem, since ‘it is a gas’, and so more-or-less follows the ideal gas laws.
So … you can do that last part yourself. 1.20 divided by 22.41
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