The number of moles of argon that must be released in order to drop.
Solution:
Initial Temperature = 25°c = 298 K
Final Temperature =125 °c = 398 K
Initial Moles (n1) = 0.40 mole
Now, Using the ideal gas law,
n1T1 = n2T2
0.400×298 = n2 × 398
n2 = 0.299 mol
Moles of Argon released
= 0.400-0.299
= 0.100 mol.
Pressure and force are related. That is using the physical equations if you know the other, you can calculate one using pressure = force/area. This pressure can be reported in pounds per square inch, psi, or Newtons per square meter N/m2. Kinetic energy causes air molecules to move faster. They hit the walls of the container more often and with greater force. The increased pressure inside the can may exceed the strength of the can and cause an explosion.
Learn more about The temperature here:-brainly.com/question/24746268
#SPJ1
Answer:
damming rivers for hydroelectricity, using water for farming, deforestation and the burning of fossil fuels.
Explanation:
The answer is cell wall...i found it here: https://www.quia.com/jg/1351880list.html
Answer:
After increasing the volume, we have 1.81 moles of hydrogen gas in the container
Explanation:
Step 1: Data given
Number of moles hydrogen gas (H2) = 1.24 moles
Volume of hydrogen gas (H2° = 27.8 L
The final volume is increas to 40.6 L
Step 2: Calculate the new number of moles
V1/n1 = V2/n2
⇒with V1 = the initial volume = 27.8 L
⇒with n1 = the initial number of moles H2 = 1.24 moles
⇒with V2 = the final volume = 40.6 L
⇒with n2 = the new number of moles = TO BE DETERMINED
27.8L / 1.24 moles = 40.6 L / n2
n2 = 40.6 / (27.8/1.24)
n2= 1.81 moles
After increasing the volume, we have 1.81 moles of hydrogen gas in the container