When 11.0 g of zinc metal reacts with excess HCl, how many liters of H 2 gas are
ID: 692611 • Letter: W
Question
When 11.0 g of zinc metal reacts with excess HCl, how many liters of H2 gas are produced at STP? Express your answer to three significant figures. Do not include units in your answer.
2.) Heat of formation for CO is -110.5 KJ/mol and the heat of formation for MgO is -602 KJ/mol. Which of the following statements is true?
Impossible to determine to given data.
The bonds in MgO and CO are equally strong.
The bond in MgO is stronger than the bond in CO.
The bond in CO is stronger than the bond in MgO.
a.Impossible to determine to given data.
b.The bonds in MgO and CO are equally strong.
c.The bond in MgO is stronger than the bond in CO.
d.The bond in CO is stronger than the bond in MgO.
Explanation / Answer
1)
Molar mass of Zn = 65.38 g/mol
mass of Zn = 11.0 g
we have below equation to be used:
number of mol of Zn,
n = mass of Zn/molar mass of Zn
=(11.0 g)/(65.38 g/mol)
= 0.1682 mol
the reaction taking place is:
Zn + 2 HCl —> ZnCl2 + H2
moles of H2 formed = moles of Zn reacted
= 0.1682 mol
molar volume at STP = 22.4 L/mol
SO,
volume = number of mol * molar volume
= 0.1682 mol * 22.4 L/mol
= 3.77 L
Answer: 3.77 L
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