Answer:
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Answer:
0.1077 grams
Explanation:
First we will employ the ideal gas law to determine the number of moles of nitrogen gas.
PV=nRT
P=2 atm
V=20L
R=0.08206*L*atm*mol^-1*K^-1
T=323.15 K
Thus, 2atm*20L=n*0.08206*L*atm*mol^-1*K^-1*323.15K
K, atm, and L cancels out. Thus n=2*20mol/0.08206*323.15=1.5 moles
Lastly, we must convert the number of moles to grams. This can be done by dividing the number of moles by the molar mass of nitrogen gas, which is 14 grams.
1.5/14=0.1077 grams
<h3>
Answer:</h3>
18.65 L
<h3>
Explanation:</h3>
We are given;
- Initial volume of the container, V1 as 5.43 L
- Initial pressure of the container, P1 as 7.97 atm
- New pressure, P2 is 2.32 atm
We are required to calculate the container's new volume;
We are going to use Boyle's law
- According to Boyle's law the volume of a fixed mass of a gas and the pressure are inversely proportional at a constant absolute temperature.
- That is;

- At varying pressure and volume at constant temperature, k is the constant.
- Therefore;

Rearranging the formula;



Therefore, the new volume will be 18.65 L