For the reaction, calculate how many moles of the product form when 2.73{\rm mol} of \rm H_2 completely reacts.
Assume that there is more than enough of the other reactant.
{\rm{H}}_2 \left( g \right) + {\rm{Cl}}_2 \left( g \right)\; \rightarrow \;2\;{\rm{HCl}}\left( g \right)

Question

For the reaction, calculate how many moles of the product form when 2.73{\rm mol}  of \rm H_2 completely reacts. 
Assume that there is more than enough of the other reactant.
{\rm{H}}_2 \left( g \right) + {\rm{Cl}}_2 \left( g \right)\; \rightarrow \;2\;{\rm{HCl}}\left( g \right)

anonymous · Answer

1st find moles of HCL...by using mole ratio....moles of hcl= moles of h2 multiplied by (mole ratio)...and uhh can you right an equation for this....i'll just assume that this is the equation......H2 + 2Cl = 2HCl.....so solve like this...moles of h2 = 2.73 multiplied by 2/1....moles of h2 = 5.46 mol......if i am wrong someone plz correct me...but if that's the equation then....no prob :)