Solution:-
we will solve this question by using the Ideal Gas equation PV= nRT
Here the given Data
As the volume of the container remains the same So V= constant
So here V and R constant, So we can write
⇒ P ∝ nT
⇒
Given
Using the above formula, we can write
⇒
⇒
⇒
⇒
If 1.24 moles of H2 produces a pressure of 1.08 atm in a 4.50 L container...
12. (6 pts.) A 4.50 L container filled with argon (Ar) gas has a pressure of 1.25 atm and a temperature of 35.0 "C. Calculate the moles of Ar in the container: a. b. What would be the pressure of the container if the temperature is increased to 45.0 °C? 8 | Page
Please help with these two
1. A flask is filled with 1.08 moles of a gas at 20.7 K and
646.8 mm Hg. The flask is then opened and an additional 1.33 moles
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