I am not great at this stuff, but you need to start by writing out how many of each element there are in the product and in the reactions. It is a lot of math and trying to make the equal on both sides
have a look at the picture i’ve attached to see if it helps, let me know if you want me to go over it in more detail and i will tomorrow morning :)
Answer:
true
Explanation:
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Answer:
The answer to your question is 12
Explanation:
Data
Number of electrons in Phosphorus 3+ ion
Process
1.- The sign of the number after the name indicates if the element has lost or gained electrons.
If the sign is positive the element has lost electrons
If the sign is negative the element has gained electrons.
2.- Phosphorus atomic number is 15, then the number of electrons in Phosphorus 3+ will be 12, in this example, Phosphorus lost 3 electrons.
Taking into accoun the STP conditions and the ideal gas law, the correct answer is option e. 63 grams of O₂ are present in 44.1 L of O2 at STP.
First of all, the STP conditions refer to the standard temperature and pressure, where the values used are: pressure at 1 atmosphere and temperature at 0°C. These values are reference values for gases.
On the other side, the pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:
P×V = n×R×T
where:
- P is the gas pressure.
- V is the volume that occupies.
- T is its temperature.
- R is the ideal gas constant. The universal constant of ideal gases R has the same value for all gaseous substances.
- n is the number of moles of the gas.
Then, in this case:
- P= 1 atm
- V= 44.1 L
- n= ?
- R= 0.082
- T= 0°C =273 K
Replacing in the expression for the ideal gas law:
1 atm× 44.1 L= n× 0.082 × 273 K
Solving:
n=1.97 moles
Being the molar mass of O₂, that is, the mass of one mole of the compound, 32 g/mole, the amount of mass that 1.97 moles contains can be calculated as:
= 63.04 g ≈ <u><em>63 g</em></u>
Finally, the correct answer is option e. 63 grams of O₂ are present in 44.1 L of O2 at STP.
Learn more about the ideal gas law:
