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Report (any type)/Brief report
22/09/2021
The reaction releases 7.71 L of ##”H”_2##.
Here are the steps to follow:
First, write the balanced equation for the reaction.
Use the molar mass to convert grams of ##”Mg”## to moles of ##”Mg”##.
Use the molar ratio between ##”Mg”## and ##”H”_2## to get the moles of ##”H”_2##.
Finally, use the molar volume to convert moles of ##”H”_2## to litres of ##”H”_2##
.
Let’s see how this works.
1. The balanced equation is
##”Mg” +”2HCl” → “MgCl”_2 + “H”_2##
2. Calculate the moles of ##”Mg”##.
##8.25 color(red)(cancel(color(black)(“g Mg”))) × “1 mol Mg”/(24.31 color(red)(cancel(color(black)(“g Mg”)))) = “0.339 mol Mg”##
3. Calculate the moles of ##”H”_2##
The balanced equation tells us that ##”1 mol Mg”## gives ##”1 mol H”_2##. So,
##0.339 color(red)(cancel(color(black)(“mol Mg”))) × (“1 mol H”_2)/(1 color(red)(cancel(color(black)(“mol Mg”)))) = “0.339 mol H”_2##
4. Calculate the volume of ##”H”_2##
STP is defined as 0 °C and 1 bar.
Under these conditions, the volume of 1 mol of an ideal gas is 22.711 L.
To convert moles to litres at STP, we use the relation
##”22.711 L = 1 mol”##.
So,
##0.339 color(red)(cancel(color(black)(“mol H”_2))) × (“22.711 L H”_2)/(1 color(red)(cancel(color(black)(“mol H”_2)))) = “7.71 L H”_2##
Notice how we always write the conversion factors so that the units cancel to give the desired units for the answer.
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I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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