Water can be formed from the stoichiometric reaction of hydrogen with oxygen: $2H_2(g) + O_2(g) + 2H_2O(g)$ . A complete reaction of 5.0 g of $O_2$ with excess hydrogen produces how many grams of $H_2O$ ?

Question

13528 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-01-16T16:55:05

Your equation specifies that $32*g$ of dioxygen and $4*g$ of dihydrogen give $36*g$ of water upon reaction, so..........

$2H_2(g) + O_2(g) rarr 2H_2O(g)$

We started with $(5.0*g)/(32.00*g*mol^-1)=0.156*mol" dioxygen"$ .

Given excess dihydrogen, this molar quantity thus gives $2xx0.156*mol$ water.

And thus, $2xx0.156*molxx18.01*g*mol^-1~=6*g$ water are evolved. Is this reaction exothermic or endothermic?

Water can be formed from the stoichiometric reaction of hydrogen with oxygen: 2H_2(g) + O_2(g) + 2H_2O(g)2H_2(g) + O_2(g) + 2H_2O(g). A complete reaction of 5.0 g of O_2O_2 with excess hydrogen produces how many grams of H_2OH_2O?