At a temperature of 30 deg C, the vapour pressure of water
H2O is about 32 mm Hg. Therefore at a total pressure f 734 mm Hg, the partial
pressure of the Hydrogen gas collected is:
<span>P Hydrogen = 734 mm Hg – 32 mm Hg = 702 mm Hg</span>
Answer:
Pure solids or liquids are excluded from the equilibrium expression because their effective concentrations stay constant throughout the reaction. The concentration of a pure liquid or solid equals its density divided by its molar mass.
Explanation:
Hope this helps!!!
Answer: Volume would be 196.15 mL if the temperature were changed to and the pressure to 1.25 atmospheres.
Explanation:
Given: , = 256 mL,
= 720 torr (1 torr = 0.00131579 atm) = 0.947368 atm
,
Formula used to calculate volume is as follows.
Substitute the values into above formula as follows.
Thus, we can conclude that the volume would be 196.15 mL if the temperature were changed to and the pressure to 1.25 atmospheres.
Heat & pressure. hope this helps