To solve this problem, we need to use stoichiometry to find the number of moles of hydrogen gas produced, and then convert that to volume using the given information.
First, let's calculate the number of moles of zinc (Zn) used in the reaction. The molar mass of zinc (Zn) is 65.1 g/mol.
Number of moles of Zn = mass of Zn / molar mass of Zn
Number of moles of Zn = (2 * 60 g) / 65.1 g/mol
Number of moles of Zn = 1.847 moles
According to the balanced equation, 1 mole of zinc reacts to produce 1 mole of hydrogen gas (H2). Therefore, the number of moles of hydrogen gas produced is also 1.847 moles.
Now let's convert the number of moles of hydrogen gas to volume at STP. 1 mole of any gas occupies 22.4 dm3 at STP.
Volume of hydrogen gas = number of moles of H2 * 22.4 dm3/mol
Volume of hydrogen gas = 1.847 moles * 22.4 dm3/mol
Volume of hydrogen gas = 41.2976 dm3
Therefore, the volume of hydrogen gas produced at STP when 2 * 60 g of zinc reacts with excess HCl is 41.3 dm3.
What volume of hydrogen is produced at STP when 2•60g of zinc reacts with excess HCl according to the equation below
Zn+2HCL>ZnCl+H2
Zn=65,1 mole of a gas occupies 22•4 dm3 at STP.
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