The number of moles of HCl in an aqueous hydrochloric acid solution can be determined as follows moles=(concentration in M units) (Volume in liters)
for example - in 10.00 ml of 10 M HCI, the number of moles is: moles = (10 moles/L) (0.0100 L) = 0.10 moles
Using this method, which of the follow is correct for the Zn+HCl reaction? we were asked to mix 2 g of Zn with 10ml of HCL
1) HCl reagent was added in excess
2) HCl was the limiting reagent
3) Zn and HCl were added in the stoichiometric amounts
4) The reaction stoichiometry of Zn and HCl cannot be determined

1) HCl reagent was added in excess

Explanation:

The equation of the reaction is given as;

Zn + HCl --> ZnCl2 + H2

From the stoichiometry;

1 mol of Zn reacts with 1 mol of HCl

In 2g of Zn;

mass = 2

Molar mass = 65.38g/mol

Number of moles = Mass/ Molar mass = 2 / 65.38 = 0.03059 mol

In 10ml of HCl;

the number of moles is: moles = Concentration * Volume =  (10 moles/L) (0.0100 L) = 0.10 moles

Comparing 0.03059 mol  of Zn : 0.10 mol of HC with the stochiometry, we can deduce that HCl is by far greater. Hence the correct option is option 1.

b.

the accuracy of the data.

4d^55s^1 ( third choice)