How many moles of oxygen gas are consumed in the production of 5.00 g of iron(III) oxide from metallic iron? 4Fe(s)+3O2(g)→2Fe2O3(g) mole(s) O2

0.0469 mol of 02.

Explanation:

The balanced equation of this reaction is given as follows:

4Fe(s) + 3O2(g) → 2Fe2O3(s)

According to this equation, 3 moles of oxygen gas (O2) is consumed to produce 2 moles of iron(III) oxide (Fe2O3).

Using the formula, mole = mass/molar mass to convert mass of Fe2O3 to mole

Molar mass of Fe2O3 = 56(2) + 16(3)

= 112 + 48

= 160g/mol

mole = 5.00 g ÷ 160g/mol

mole = 0.03125mol of Fe2O3

Since 3 moles of oxygen gas (O2) is consumed to produce 2 moles of iron(III) oxide (Fe2O3).

0.03125mol of Fe2O3 will be produced when (0.03125 × 3/2) mol of oxygen gas is consumed.

0.03125 × 3/2

0.03125 × 1.5

= 0.0469 mol of 02.

answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.