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
Ionicly
They do not share electrons. All of the electrons get attracted the the group 7 element and they stick together electrostaticly.
Answer:
Chemicals
Explanation:
Chemistry is the study if chemicals and chemical reactions, atoms, etc
Answer
Third option 1 L = 1.06 qt
Explanation
The quart (symbol: qt) is a unit of volume, a liquid quart is equal to approximately 0.946353 liters and a dry quart is equal to approximately 1.101221 liters.
Answer:
[Ba^2+]= 0.400M
[OH-]= 0.800M
Explanation:
Step 1: Data given
Molarity ofBa(OH)2 = 0.400 M
Ba(OH)2 is a strong electrolyte, so 100 % dissociation
Step 2: The equation
Ba(OH)2 → Ba^2+ + 2OH-
In 1 mol Ba(OH)2 we have 1 mol Ba^2+ and 2 moles OH-
Step 3: Calculate the concentration
[Ba^2+]= 1* 0.400 M = 0.400M
[OH-]= 2*0.400 M = 0.800M