See Figure 4 below.
1. Draw a 7-carbon chain and number the carbon atoms (<em>Figure 1</em>).
2. Insert a triple bond between atoms 5 and 6 (<em>Figure 2</em>).
3. Attach a phenyl group to atom 3 (<em>Figure 3</em>).
4. Attach a Br to atom 1 (Figure 4).
And you have your structure.
<em>Note</em>: The C≡C triple bond takes <em>priority</em> in the naming, so we must number the chain from the other end. The correct name is
<em>7-bromo-5-phenylhept-2-yne </em>(all one word).
1.31 × 10⁴ grams.
<h3>Explanation</h3>Assume that oxygen acts like an ideal gas. In other words, assume that the oxygen here satisfies the ideal gas law:
,
where
Apply the ideal gas law to find :
.
In other words, there are 410.3 moles of O₂ molecules in that container.
There are two oxygen atoms in each O₂ molecules. The mass of mole of O₂ molecules will be . The mass of 410.3 moles of O₂ will be:
.
What would be the mass of oxygen in the container if the pressure is approximately the same as STP at or
instead?