CHEMISTRY QUESTION PLEASE HELP?
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table.
Total volume of H2(g) collected 93.13 mL
Temperature 28.0 °C
Barometric pressure 7.40×102 mmHg
Vapor pressure of water at 28.0 °C 28.5 mmHg
Calculate the moles of hydrogen gas produced by the reaction.
- hcbiochemLv 73 weeks agoBest Answer
Subtracting the vapor pressure of water from the barometric pressure will give you the partial pressure of H2 collected:
P = 740 - 28.5 = 711.5 mm Hg / 760 = 0.936 atm H2
Now, use the ideal gas law to calculate moles H2:
PV = n RT
0.936 atm (0.09313 L) = n (0.08206 Latm/mol K) (301 K)
n = 3.53X10^-3 mol H2