The first thing you need to do is figure out how many Hydrogen atoms there are in just one propant molecule. You can do this just by looking at the formula, there are 8 Hydrogens. So now you know for each propant molecule, you have 8 Hydrogens.Moe_slow said:
then i multiply that by 6.02 x 10^23 to give me the number of molecules?...what do i do from there if have done everything correctly so far? do i divide that by 8? to give me the number of molecules of Hydrogen
I would multiply by 8, not divide.Moe_slow said:
\Also, multiply by the molar quantity of that element in a mole of that compoundMoe_slow said:
Right, you convert to a mole ratio as:Moe_slow said:
As 100% - 45.6% = 55.4%, you can solve asMoe_slow said:
Primarily done to increase each component (of the ratio) to be equal to or greater than one (1),Moe_slow said:
bomba923 said:Right, you convert to a mole ratio as:
As 100% - 45.6% = 55.4%, you can solve as
[tex]\left( {\frac{{{\text{171g}}\;{\text{Ba}}\left( {{\text{OH}}} \right)_2 }}
{{{\text{1}}\,{\text{mol}}\;{\text{Ba}}\left( {{\text{OH}}} \right)_2 \cdot n{\text{H}}_2 {\text{O}}}}} \right)\left( {\frac{{1.000{\text{g Ba}}\left( {{\text{OH}}} \right)_2 \cdot n{\text{H}}_2 {\text{O}}}}{{0.554{\text{g}}\;{\text{Ba}}\left( {{\text{OH}}} \right)_2 }}} \right)\left( {\frac{{0.456\,{\text{g}}\;{\text{H}}_{\text{2}}{\text{O}}}}{{1.000{\text{g Ba}}\left( {{\text{OH}}} \right)_2 \cdot n{\text{H}}_2 {\text{O}}}}} \right)\left( {\frac{{{\text{1}}\,{\text{mol}}\;{\text{H}}_2 {\text{O}}}}{{18.0{\text{g}}\;{\text{H}}_2 {\text{O}}}}} \right) = \frac{{7.8\,{\text{mol}}\;{\text{H}}_{\text{2}} {\text{O}}}}{{1\,{\text{mole}}\;{\text{Ba}}\left( {{\text{OH}}} \right)_2 \cdot n{\text{H}}_2 {\text{O}}\;}}[/tex]
[tex] \approx \frac{{8\,{\text{mol}}\;{\text{H}}_{\text{2}} {\text{O}}}}
{{1\,{\text{mole}}\;{\text{Ba}}\left( {{\text{OH}}} \right)_2 \cdot n{\text{H}}_2 {\text{O}}}}[/tex]
And so, the molecular formula of your hydrate is:
[tex]{\text{Ba}}\left( {{\text{OH}}} \right)_2 \cdot 8{\text{H}}_2 {\text{O}}[/tex]
A mole is a unit of measurement used in chemistry to represent the amount of a substance. One mole is equal to Avogadro's number, which is approximately 6.02 x 10^23.
A mole is different from other units of measurement because it represents a specific number of particles, rather than a specific amount of mass or volume. This makes it useful for comparing the number of atoms or molecules in different substances.
To convert between moles and other units, you will need to know the molar mass of the substance. You can find this by adding up the atomic masses of all the elements in the substance. Then, to convert from moles to grams, multiply the number of moles by the molar mass. To convert from grams to moles, divide the number of grams by the molar mass.
In chemical equations, moles are used to show the ratio between different substances. The coefficients in a balanced chemical equation represent the number of moles of each substance involved in the reaction. This allows chemists to accurately predict the amount of products that will be formed from a given amount of reactants.
Understanding moles is important in chemistry because it allows us to accurately measure and compare the amounts of different substances. This is crucial for making accurate predictions and carrying out experiments in the lab. It also helps us to better understand the composition and behavior of substances at the atomic and molecular level.