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February 5, 2016
Posted by **Yuli** on Thursday, November 24, 2011 at 12:14am.

Zn(s)+ 2HCl(aq)---> ZnCl2(aq)+ H2(g)

Data:

Mass of vial and zinc 15.5082

mass of vial 15.3972

mass of zinc 0.111

final burette reading 45.30mL

barometric pressure: Patm 100.6kPa

temperature of trapped gas 24.3C

vapour pressure of water at 24.3 C: PH2O 3.004kPa

diff in solution lvls inside and outside burette 162mm H2O

I got 95.968 kPa of H2 since you said im allowed 4 sigfig i used 95.97 does that seem right?

and for the second part i got 297.5K im really not sure what am doing here the formulas i was trying to use were

atm = H2+ H2O+ lvldiff

H2= atm- lvldiff-H2O

- chemistry -
**DrBob222**, Thursday, November 24, 2011 at 12:45amLet's see. I said we should take

100.6 kPa - vp H2O - water diff or

100.6 - 3.004 - 1.5876 = 96.008 kPa which rounds to 96.00 to 4 s.f. How does that stack up with the formula you are using.

atm = H2 + H2O + |v| or

H2 = atm - H2O - |v| or

H2 = 100.6 - 3.004 - 1.5876 = 96.008 and it rounds to 96.00 kPa. (I didn't use a formula; I just reasoned it out but I'm glad to see that reasoning and the formula gets the same thing. Check your math. I don't believe 95.968 kPa is correct.

- chemistry -
**Yuli**, Thursday, November 24, 2011 at 12:55amhow would you calculate the temperature of H2 in kelvin? and the moles that H2 produced? do you know a formula for that? could you please explain it to me thanks for all your help so far i've understood everything thanks to you.

- chemistry -
**DrBob222**, Thursday, November 24, 2011 at 1:20amYour post says temperature of trapped gas is 24.3 C. In kelvin, that is 273.15+24.3 = 297.45. I would round that to 297.4; however, when I'm doing calculations, I can make "rounding" errors; therefore, I leave all of the numbers in my calculator and go to the next calculation. I also carry one more place than I'm allowed to avoid rounding errors, then round at the very end of all calculations.You can calculate moles H2 from PV = nRT. You know P now, you know V(must be in liters), you know R (it's 8.314 if you use P in kPa) and you know T in kelvin. Solve for n.

- chemistry -
**Yuli**, Thursday, November 24, 2011 at 1:52amI did all my questions but there is this last one i dont get. Calculate the number of moles of zinc that must have reacted( assume that Zn is limiting and the yield of H2 gas is 100%) how do you do this? could you help me with this last one please?

- chemistry -
**DrBob222**, Thursday, November 24, 2011 at 12:49pmmoles Zn = grams Zn/atomic mass Zn