Write a question you have about Titan or about methane that could help you determine what happened to the lake
1 answer:
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Answer:
a. 167 mL.
b. 39.3 %.
Explanation:
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In this case, for the undergoing chemical reaction, since 45.0 g of aluminum react, based on the 2:3 mole ratio with sulfuric acid, we can compute the required moles as shown below:
Next, since the molarity of a solution is computed based on the moles and volume (M=n/V), we can compute the required volume of sulfuric acid as shown below:
That in mL is 167 mL.
Moreover, for the percent yield, we compute the grams of aluminum sulfate that are produced based on the required 2.50 moles of sulfuric acid:
Therefore the percent yield is:
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Answer:
.
Explanation:
<h3>Step One: calculate the coefficients. </h3>Look up the relative atomic mass of these four elements on a modern periodic table:
: approximately
.
: approximately
.
: approximately
.
: approximately
.
The relative atomic mass of an element is numerically equal to the mass (in grams, ,) of one mole of atoms of this element.
For example, the relative atomic mass of is approximately
. Therefore, each mole of
atoms would have a mass of
.
This sample contains of carbon. That would correspond to approximately
of
atoms.
Similarly, for the other three elements:
.
.
.
Hence, the ratio between these elements in this compound would be:
.
In the empirical formula of a compound, the coefficients should represent the smallest possible integer ratio between the number of atoms of these elements.
is indeed the smallest possible integer ratio between the number of atoms of these elements.
Apply the Hill System to arrange these four elements in the empirical formula. In the Hill System:
If carbon, , is present in this compound, then:
- The other elements in this compound will be listed in alphabetical order.
If there is no carbon in this compound, then list all the elements in this compound in alphabetical order.
Both (carbon) and
(hydrogen) are found in this compound. Therefore, the first element in the list would be
. The second would be
, followed by
and then
.
Hence, the empirical formula of this compound would be .