How many grams of hydrogen gas will be liberated when 6g of magnesium ribbon dissolves in 500cm3 of 6M HCl?
(Mg=24, H=1, Cl=35.5)
1.2 g
0.7 g
0.5 g
0.3 g
0.12 g
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Myschool is taking a rather long process
Simply,
According to the equation: 2HCl + Mg ------ MgCl2 + H2
24g of magnesium ribbon liberates 2g of hydrogen gas from HCl, if 24g liberates 2g, how many grams of hydrogen will be liberates from 6g of magnesium?
24g ----> 2g
6g ----> x
24x = 6×2
x = 12/24 = 0.5g
very simple to solve, dont need to go through all these workings just go like this
2Hcl+mg---->mgcl +H2
1 mole of mg=2g of hydrogen
and 6g/24g of magnsium gives 0.25moles
now
1 mole of mg=2g of hydrogen
0.25moles of mg =?
cross multiple 0.25*2g =0.5g
To get the mole of HCL
mole= conc.×volume/1000
= 500×6/1000 = 3
3 mole of hydrogen chloride divide by 6 gram of magnesium ribbon to get the mass of hydrogen chloride = 3/6 = 0.5
🥺 do anybody have an explanation for this problem
I was giving a wrong result, i scored 8 out of 10 not 7 out of 10. Please kindly correct the mistake
THANK YOU, FOR YOUR UNDERSTANDING
