How many moles of oxygen must be placedin a 3.00 L container to exert a pressure of 2.00 atm at 25.0°C?
Which variables are given?
Answers
0.24 moles of oxygen must be placed in a 3.00 L container to exert a pressure of 2.00 atm at 25.0°C.
The variables given are Pressure, volume and temperature.
Explanation:
Given:
P = 2 atm
V = 3 litres
T = 25 degrees or 298.15 K by using the formula 25 + 273.17 = K
R = 0.082057 L atm/ mole K
n (number of moles) = ?
The equation used is of Ideal Gas law:
PV = nRT
n =
Putting the values given for oxygen gas in the Ideal gas equation, we get
n =
= 0.24
Thus, from the calculation using Ideal Gas law it is found that 0.24 moles of oxygen must be placed in a container.
Ideal gas law equation is used as it tells the relation between temperature, pressure and volume of the gas.
Answer:
0.245 on Ed
Explanation:
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The subscript 2 on the Bromine, Br atom simply means Magnesium ion is; Mg²+.
Discussion:
When magnesium ion, Mg²+ combines with an halogen like Bromine, Br-.
In such scenario, there must be a balance of charges for the formation of a compound like MgBr2.
As such, 2 Br- ions and 1 Mg²+ are necessary to maintain charge balance in the compound.
Read more:
Final answer:
The '2' in Magnesium bromide (MgBr2) represents the 2 bromide ions that associate with each magnesium ion in the ionic compound, ensuring overall neutrality.
Explanation:
In the ionic compound Magnesium bromide (MgBr2), the '2' signifies the number of bromine (Br) atoms that are combined with a single atom of Magnesium (Mg) to form this compound. This is due to the fact that magnesium (Mg) has two valence electrons which it donates to form a stable compound, resulting in a Mg2+ cation. The bromine atom accepts one electron to form a Br- anion. Since Mg needs to donate two electrons, two Br ions are required, which gives us the '2' in MgBr2. This ratio of ions ensures neutrality of the overall ionic compound.
Learn more about Ionic Compounds here:
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