A piece of zinc metal was put in 200 mL of 0.10 M HCl solution. A tiny piece of zinc which weighed 0.096 g was left after the reaction. The reaction takes place as: Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g) Calculate the followings: Moles HCl reacted Moles of Zn reacted Mass of the original zinc piece used Number of H2 molecules produced Volume of H2 at STP.
A piece of zinc metal was put in 200 mL of 0.10 M HCl solution. A tiny piece of zinc which weighed 0.096 g was left after the reaction. The reaction takes place as: Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g) Calculate the followings: Moles HCl reacted Moles of Zn reacted Mass of the original zinc piece used Number of H2 molecules produced Volume of H2 at STP.
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A piece of zinc metal was put in 200 mL of 0.10 M HCl solution. A tiny piece of zinc which weighed 0.096 g was left after the reaction. The reaction takes place as:
Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g)
Calculate the followings:
- Moles HCl reacted
- Moles of Zn reacted
- Mass of the original zinc piece used
- Number of H2 molecules produced
- Volume of H2 at STP.
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