Write down the Balanced reaction equation.
Zn +2HCl = ZnCl2 + H2
The Molar ratios are 1:2::1:1
So one mole of Zinc requires two moles of Hydrochloric Acid for complete reaction, where both reactants are completely used.
So for example if you had only 0.5 moles zinc and two moles of HCl, then zinc would be the limiting reactant , because all the zinc will be used up leaving 1 mole of HCl unreacted .
The molar ratios are not equal 0.5 : 2 :: 0.5 : 0.5 (Leaving 2 - 1 = 1 mole HCl )
Conversely if you had 1 mole zinc and only one mole of HCl, then HCl would be the limiting reactant, because all the HCl would be used up leaving o.5 (Half) a mole of zinc unreacted.
Similarly
1:1:: 0.5 : 0.5 leaving (1 - 0.5 = 0.5 mole zinc)
It all requires the moles to be in the correct ratios.
In this reaction zinc is the limiting reactant.
Iodide.
The balanced equation is as follows: Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g)
Zn + 2HCl --> ZnCl2 + H2
Yes, according to the equation Zn (s) + 2HCl (aq) ----> ZnCl2 (aq) + H2 (g).
2HCl + Zn --> ZnCl2 + H2
The reaction is: Zn + 2HCl = ZnCl2 + H2
The balanced equation is as follows: Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g)
The net ionic equation is Zn + 2H+ --> Zn2+ + H2
Zn + 2HCl --> ZnCl2 + H2
yes Zn + 2HCl -> ZnCl2 + H2 is balanced
Zn + 2HCl --- ZnCl2 + H2 Mg + 2HCl --- MgCl2 + H2
Yes, according to the equation Zn (s) + 2HCl (aq) ----> ZnCl2 (aq) + H2 (g).
Zn + 2HCl -> ZnCl2 + H2
2HCl + Zn --> ZnCl2 + H2
Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(gas)
2HCl + Zn -----> ZnCl2 + H2
The reaction is: Zn + 2HCl = ZnCl2 + H2
Zn + 2HCl -> ZnCl2 +H2