Answer:
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28.4 grams of P₂O₅ will be obtained from the interaction of 11.2 liters of oxygen with phosphorus.
Let's consider the following balanced equation.
4 P + 5 O₂ ⇒ 2 P₂O₅
Since the conditions are not specified, we will assume that we are working at standard temperature and pressure. At STP, 1 mole of an ideal gas occupies 22.4 L. The volume of 11.2 L of oxygen at STP, assuming ideal behavior, is:
The molar ratio of O₂ to P₂O₅ is 5:2. The moles of P₂O₅ obtained from 0.500 moles of O₂ are:
The molar mass of P₂O₅ is 141.94 g/mol. The mass corresponding to 0.200 moles of P₂O₅ is:
28.4 grams of P₂O₅ will be obtained from the interaction of 11.2 liters of oxygen with phosphorus.
You can learn more about stoichiometry here: brainly.com/question/22288091
These metals are silver and soft, much like the alkali metals of Group 1. These metals also react with water, though not as vigorously. Beryllium, interestingly, does not react with water. Each alkaline earth metal has two valence electrons.
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