Answer:
B. 75.0 kPa
Explanation:
P1V1/T1=P2V2/T2
(x * 100 L)/(300 K)=(100 kPa * 50.0 L)/(200 K)
x=75.0 kPa
Answer:
number of moles of
=4.16mol
Explanation:
experiment data:
temperature=
=273+22 k=295k
pressure=1.007 atm
volume is missing so assuming volume-=100L
using ideal law relationship
ideal gas means gas which occupies negligible space and there is no interaction between the molecules of gases.
PV=nRT
put all the experimental data, we get
n=4.15 mol
number of moles of
=4.16mol
Answer:
Total pressure = 1109.2 torr
Explanation:
Given data:
Partial pressure of cyclopropane = 334 mmHg
Partial pressure pressure of oxygen = 1.02 atm
Total pressure of mixture = ?
Solution:
Formula:
Total pressure = P of C₃H₆ + P of O₂
1 atm = 760 torr = 760 mmHg
1.02 atm × 760 torr / 1atm = 775.2 torr
Total pressure = P of C₃H₆ + P of O₂
Total pressure = 334 torr + 775.2 torr
Total pressure = 1109.2 torr
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Things expand when heated. therefore the molecules are farther apartand the matierial is less dense. Things expand because their molecules are vibrating faster and are taking up more space