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b. Determine the pressure of the hydrogen gas collected (in atm) at ( 298 mathrm{~K} ), given the height of the remaining column of liquid in the buret was measured to be ( 174 mathrm{~mm} ) and the barometric pressure was ( 741.6 mathrm{~mm} mathrm{Hg} ). You will need to refer to data in Table I of the experiment for the vapor pressure of water. Hint: Note: [ P_{mathrm{H}_{2}}=P_{ ext {barometric }}-P_{ ext {hydrostatic }}-P_{mathrm{H}_{2} mathrm{O}} ] and [ P_{ ext {hydrostatic }}=frac{ ext { height of liquid in buret in } mathrm{mm}}{left(13.6 frac{mathrm{mmH}_{2} mathrm{O}}{mathrm{mmHg}} ight)} ] atm c. Use the ideal gas law to find the number of moles of hydrogen gas. Hint: [ mathrm{mol} mathrm{H}_{2}(g) ] 4. If the initial mass of the anode was ( 22.814 mathrm{~g} ) and the final mass was ( 22.746 mathrm{~g} ), determine the number of moles of copper oxidized. mol

          b. Determine the pressure of the hydrogen gas collected (in atm) at ( 298 mathrm{~K} ), given the height of the remaining column of liquid in the buret was measured to be ( 174 mathrm{~mm} ) and the barometric pressure was ( 741.6 mathrm{~mm} mathrm{Hg} ). You will need to refer to data in Table I of the experiment for the vapor pressure of water. Hint:
Note:
[
P_{mathrm{H}_{2}}=P_{	ext {barometric }}-P_{	ext {hydrostatic }}-P_{mathrm{H}_{2} mathrm{O}}
]
and
[
P_{	ext {hydrostatic }}=frac{	ext { height of liquid in buret in } mathrm{mm}}{left(13.6 frac{mathrm{mmH}_{2} mathrm{O}}{mathrm{mmHg}}
ight)}
]
atm
c. Use the ideal gas law to find the number of moles of hydrogen gas. Hint:
[
mathrm{mol} mathrm{H}_{2}(g)
]
4. If the initial mass of the anode was ( 22.814 mathrm{~g} ) and the final mass was ( 22.746 mathrm{~g} ), determine the number of moles of copper oxidized.
mol

$b. Determine the pressure of the hydrogen gas collected (in atm) at ( 298 mathrm K ), given the height of the remaining column of liquid in the buret was measured to be ( 174 mathrm mm ) and the barometric pressure was ( 741.6 mathrm mm mathrmHg ). You will need to refer to data in Table I of the experiment for the vapor pressure of water. Hint: Note: [ PmathrmH2=P ext barometric -P ext hydrostatic -PmathrmH2 mathrmO ] and [ P ext hydrostatic =frac ext height of liquid in buret in mathrmmmleft(13.6 fracmathrmmmH2 mathrmOmathrmmmHg ight) ] atm c. Use the ideal gas law to find the number of moles of hydrogen gas. Hint: [ mathrmmol mathrmH2(g) ] 4. If the initial mass of the anode was ( 22.814 mathrm g ) and the final mass was ( 22.746 mathrm g ), determine the number of moles of copper oxidized. mol$

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