0.25g zinc & 10mL 6M HCl react. How many moles zinc reacted & how many moles H was produced.?

This is from a virtual lab. When 10 mL 6M HCl solution was added to 0.25g zinc in a flask, psi went from 14.697 to 26.610 and temp went from 21 C up to 34.85 C. After cooling to 21 C, psi = 25.413. After connecting flask to a piston, Gas vol = 102.14 mL, O2 mol = 0.000524, N2 mol = 0.002096.

0.25g zinc %26amp; 10mL 6M HCl react. How many moles zinc reacted %26amp; how many moles H was produced.?
The balanced equation is:





Zn (s) + 2 HCl (aq) --%26gt; ZnCl2 (aq) + H2 (g)





0.25 g / 65.41 g/mol = number of moles of Zn available


= 0.00382 moles





10 mL / (1000 mL/L) * 6 mole/L = number of moles of HCL available


= 0.06 moles





There is enough acid to react with all of the Zinc. Every mole of Zinc will produce one mole of Hydrogen gas, so 0.00382 moles of Hydrogen is produced.





At STP, this would produce 22.4 L/mole * 0.00382 moles = 0.0856 L of Hydrogen gas (or 85.6 mL). You can translate this using





P1V1 = P2V2 into alother Temperature and Pressure to determine error.
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