The gram-formula mass of NO2 is defined as the mass of one mole of
a. one mole of NO2
b. one molecule of NO2
c. two moles of NO
d. two molecules of NO
Explain why.
I think it's a.
its a
The gram-formula mass of a compound is defined as the mass of one mole of that compound.
In this case, the gram-formula mass of NO2 refers to the mass of one mole of NO2 molecules.
So, the correct answer is option a. one mole of NO2, because the gram-formula mass is based on the molar amount of the compound and not the individual molecules.
The gram-formula mass of a compound is defined as the mass of one mole of that compound. In this case, we are considering the gram-formula mass of NO2.
To determine the answer, we need to understand the molecular formula of NO2 and apply the definition of gram-formula mass.
The molecular formula of NO2 represents one molecule of nitrogen dioxide, which consists of one atom of nitrogen (N) and two atoms of oxygen (O). The formula indicates that there is one NO2 unit present in the compound.
Now, let's consider the options provided:
a. one mole of NO2: This option is correct because it aligns with the definition of gram-formula mass. The gram-formula mass of NO2 represents the mass of one mole of NO2.
b. one molecule of NO2: This option is incorrect. While it represents the molecular formula of NO2, the gram-formula mass definition specifies the mass of one mole of the compound.
c. two moles of NO: This option is incorrect. Although NO is related to NO2, it is a different compound. The gram-formula mass of NO2 specifically refers to NO2, not NO.
d. two molecules of NO: This option is incorrect. Similar to option c, NO is distinct from NO2. The gram-formula mass of NO2 is not the mass of two molecules of NO.
In conclusion, the correct answer is a. one mole of NO2, as it represents the mass of one mole of NO2, in accordance with the definition of gram-formula mass.