In 1901, Thomas Edison invented the nickel-iron battery. The following reaction takes place in the battery. Fe(s) + 2 NiO(OH)(s) + 2 H2O(l) Fe(OH)2(s) + 2 Ni(OH)2(aq) How many mole of Fe(OH)2, is produced when 6.00 mol Fe and 8.45 mol NiO(OH) react?
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Step 1
The given equation is already balanced: \[ \text{Fe}(s) + 2 \text{NiO(OH)}(s) + 2 \text{H}_2\text{O}(l) \rightarrow \text{Fe(OH)}_2(s) + 2 \text{Ni(OH)}_2(aq) \] Show more…
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Nickel-Iron Battery In 1901 , Thomas Edison invented the nickel-iron battery. The following reaction takes place in the battery. \begin{equation} \mathrm{Fe}(\mathrm{s})+2 \mathrm{NiO}(\mathrm{OH})(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \end{equation} \begin{equation} \quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\mathrm{Fe}(\mathrm{OH})_{2}(\mathrm{s})+2 \mathrm{Ni}(\mathrm{OH})_{2}(\mathrm{aq}) How many mol of $\mathrm{Fe}(\mathrm{OH})_{2}$ is produced when 5.00 $\mathrm{mol}$ of Fe and 8.00 $\mathrm{mol}$ of $\mathrm{NiO}(\mathrm{OH})$ react? \end{equation}
Ronald P.
For each of the following balanced chemical equations, calculate how many moles of product(s) would be produced if 0.500 mole of the first reactant were to react completely. a. $\mathrm{CO}_{2}(g)+4 \mathrm{H}_{2}(g) \rightarrow \mathrm{CH}_{4}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)$ b. $\mathrm{BaCl}_{2}(a q)+2 \mathrm{AgNO}_{3}(a q) \rightarrow 2 \mathrm{AgCl}(s)+\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)$ c. $\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{H}_{2} \mathrm{O}(l)+3 \mathrm{CO}_{2}(g)$ d. $3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{Fe}(s) \rightarrow \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+3 \mathrm{H}_{2}(g)$
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