PO2 (or gases) is measure in which unit?
a- Mmol
b- umol
c- mmHg
© mEq/L (mmol in SI) is used for electrolytes e.g. BE, bicarbonate and H+. While mmHg (or kpa in SI) is used for gases e.g. pCO2 and pO2.
-------------------------
To simplify their calculations, chemists have created a standard unit for the number of atoms of a particular compound involved in a reaction or other chemical process. They define a mole (mol) as the quantity of any substance having the same number of basic units as 12 grams of carbon 12, the Avogadro number (6.022 x 1023). The SI (metric) measurement system defines one millimole (Mmol) in thousandths of a mole. You usually calculate the number of moles of a substance by weighing the amount you have on hand. If you want to convert to Mmol, multiply by 103 (1,000).
How to calculate moles:
Atomic masses are measured in units of atomic mass (AMU). A UMA represents exactly 1/12 of the mass of the nucleus of a carbon atom 12 in its ground state. One mole of substance is defined as being equal to the number of particles of this substance Avogadro. According to this definition, the weight of one mole of a substance in grams is the same number as the weight of an individual particle of that substance in the AMU. For example, the atomic weight of carbon 12 is 12 AMU. A mole of carbon 12 therefore weighs 12 grams.
Consider a container filled with hydrogen gas (H2). Each particle in the container is a molecule composed of two hydrogen atoms. So you only need to know the atomic mass of hydrogen to calculate the molecular weight. Most versions of the periodic table list the atomic mass of each element under its symbol. For hydrogen, which has a single proton in its nucleus, it is 1,008 AMU, which is the average of all natural isotopes of hydrogen. As a result, the atomic mass of hydrogen gas is 2,016 AMU and one mole of hydrogen gas weighs 2,016 grams. To find the number of moles in your sample, weigh the sample in grams and divide that weight by the molecular weight of the gaseous hydrogen in grams. For example, a sample weighing 15 grams of pure hydrogen contains 7.44 moles.
Conversion to Mmol:
Sometimes the quantities under study are so small that it is difficult to express them in moles. Enter the millimole. By multiplying the number of moles per mile, you can convert a very small number into a more manageable number. This is especially useful when using volume units in the milliliter range.
1 mol = 1000 Mmol
Concentration of the solution:
Chemists use molarity as a measure of the concentration of a particular compound in solution. They define molarity as the number of moles per liter. You convert the molarity to millimolarity by multiplying by 1,000. For example, a solution of 1 mol (molar, also written in M) has a concentration of 1 mole per liter. This equates to a solution of 1000 mmol (millimolar, sometimes also written in mM), which contains 1000 mmol per liter.
a- Mmol
b- umol
c- mmHg
© mEq/L (mmol in SI) is used for electrolytes e.g. BE, bicarbonate and H+. While mmHg (or kpa in SI) is used for gases e.g. pCO2 and pO2.
-------------------------
To simplify their calculations, chemists have created a standard unit for the number of atoms of a particular compound involved in a reaction or other chemical process. They define a mole (mol) as the quantity of any substance having the same number of basic units as 12 grams of carbon 12, the Avogadro number (6.022 x 1023). The SI (metric) measurement system defines one millimole (Mmol) in thousandths of a mole. You usually calculate the number of moles of a substance by weighing the amount you have on hand. If you want to convert to Mmol, multiply by 103 (1,000).
How to calculate moles:
Atomic masses are measured in units of atomic mass (AMU). A UMA represents exactly 1/12 of the mass of the nucleus of a carbon atom 12 in its ground state. One mole of substance is defined as being equal to the number of particles of this substance Avogadro. According to this definition, the weight of one mole of a substance in grams is the same number as the weight of an individual particle of that substance in the AMU. For example, the atomic weight of carbon 12 is 12 AMU. A mole of carbon 12 therefore weighs 12 grams.
Consider a container filled with hydrogen gas (H2). Each particle in the container is a molecule composed of two hydrogen atoms. So you only need to know the atomic mass of hydrogen to calculate the molecular weight. Most versions of the periodic table list the atomic mass of each element under its symbol. For hydrogen, which has a single proton in its nucleus, it is 1,008 AMU, which is the average of all natural isotopes of hydrogen. As a result, the atomic mass of hydrogen gas is 2,016 AMU and one mole of hydrogen gas weighs 2,016 grams. To find the number of moles in your sample, weigh the sample in grams and divide that weight by the molecular weight of the gaseous hydrogen in grams. For example, a sample weighing 15 grams of pure hydrogen contains 7.44 moles.
Conversion to Mmol:
Sometimes the quantities under study are so small that it is difficult to express them in moles. Enter the millimole. By multiplying the number of moles per mile, you can convert a very small number into a more manageable number. This is especially useful when using volume units in the milliliter range.
1 mol = 1000 Mmol
Concentration of the solution:
Chemists use molarity as a measure of the concentration of a particular compound in solution. They define molarity as the number of moles per liter. You convert the molarity to millimolarity by multiplying by 1,000. For example, a solution of 1 mol (molar, also written in M) has a concentration of 1 mole per liter. This equates to a solution of 1000 mmol (millimolar, sometimes also written in mM), which contains 1000 mmol per liter.
Labels
Clinical Chemistry