Collected Data Zn (g) 1.9904
Zn: Pressure of H2 (torr) 1140.80
I need help with #3 please.
1. First, the data from the Zn metal reagent will be used to determine the volume of the pressure vessel. Using the Zn sample mass, calculate the number of moles of Zn (m) used in the reaction and enter below.
Zn (M) 65.39 Zn (g)= 1.9904/65.39=0.03043
2. Using the number of moles of Zn, and the mole ratio in the reaction:
Zn (m) + 2 HCl (aq) → ZnCl2 (aq) + H2 (g)
determine the number of moles of H2 produced and enter below.
1.00*0.0304=0.0304 moles H2
3. The pressure observed after reaction with Zn metal and HCl should be corrected to subtract the pressure due to water vapor present at the final system temperature (22°C). Review the information in the introduction to this experiment (page 5) if you don't recall the vapor pressure of water at 22°C.
Page 5= the vapor pressure of water is a function of temperature, and is equal to 20 torr at 22°C. This means that a closed system containing liquid water at this temperature will contain 20 torr of water vapor.
Enter the corrected pressure Pcorr = Pobs - PH2O below.