Answer:
The molecules have (a) volume and (b) attractive forces
Step-by-step explanation:
At ordinary conditions, the molecules are so far apart that the gases behave almost ideally.
However, if you use high pressure and/or low temperatures, you force the molecules to be close together.
There are <em>two competing effects</em>:
- The attractive forces become much stronger at close distances, so the volume is less than that predicted by the Ideal Gas Law.
- The volume of the molecules becomes a significant portion of the volume of the container. The molecules have less volume in which to can move around, so the pressure is higher than that predicted by the Ideal Gas Law.
Answer:
0.158L
Explanation:
From the question, we obtained the following information:
C1 = 6.84 M
V1 =?
C2 = 1.84 M
V2 = 588 mL = 588/1000 = 0.588L
Using the dilution formula C1V1 = C2V2. The original volume can calculated for as follows:
C1V1 = C2V2
6.84 x V1 = 1.84 x 0.588
Divide both side by 6.84
V1 =(1.84 x 0.588) / 6.84
V1 = 0.158L
Answer:
Hey, use this formula
Explanation:
1 mole of carbon has 6.022 × 1023 carbon atoms so what about 79.7 moles?
cross multiply and thats the answer
