The minimum amount of H2 required to reduce completely 7.95g of CuO (mol. Mass=79.5) will be= ………..??
CuO(s) + H2(g) -------> Cu(s) + H2O(l)
1 mole (79.55g) of CuO will be reduced by 1 mole (2.016g) of hydrogen gas.
Hence 7.95g of CuO is 0.10mole of CuO and this will require 0.10 mole of hydrogen = 0.2016g of hydrogen.
not sure if this is right but i think this is the ans :
h2+CuO----->H2O+Cu
no. of moles of CuO=mass/molecular mass
=7.95/79.5
=0.1moles of CuO present
no of moles of hydrogen = x(mass of H2)/2
=x/2
since they r in the ratio 1:1
therefore, 1 of h2------> 1 of cuo
x/2<------- 0.1of cuo
x=0.2 !!!= amt of h2 required !
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CuO(s) + H2(g) -------> Cu(s) + H2O(l)
1 mole (79.55g) of CuO will be reduced by 1 mole (2.016g) of hydrogen gas.
Hence 7.95g of CuO is 0.10mole of CuO and this will require 0.10 mole of hydrogen = 0.2016g of hydrogen.
not sure if this is right but i think this is the ans :
h2+CuO----->H2O+Cu
no. of moles of CuO=mass/molecular mass
=7.95/79.5
=0.1moles of CuO present
no of moles of hydrogen = x(mass of H2)/2
=x/2
since they r in the ratio 1:1
therefore, 1 of h2------> 1 of cuo
x/2<------- 0.1of cuo
x=0.2 !!!= amt of h2 required !