Question

If anyone could help I’d appreciate it

Answer 1

Answer: 2.00 mol

Explanation:

The balanced chemical equation is:

$2H_2(g)+O_2(g)\rightarrow 2H_2O(g)$  

According to stoichiometry :

2.00 moles of $H_2$ require = 1.00 moles of $O_2$

Thus 2.00 moles of $H_2$ will require=$\frac{1}{2}\times 2.00=1.00moles$  of $O_2$

Thus both will act as limiting reagents and will be fully consumed.

2.00 moles of $H_2$ will form = 2 moles of $H_2O$

Thus 2.00 moles of $H_2$ will form = $\frac{2}{2}\times 2.00=2.00moles$  of $H_2O$

  Thus 2.00 moles of $H_2O$ will be produced from the given masses of both reactants.