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Chapter 4: 4.12 CYL (page 201)

Which is the limiting reactant when 5.00 g of H2 and 10 g of O2 react to form water?

Short Answer

Expert verified

O2 is the limiting reactant

Step by step solution

01

Calculating moles of both of them

The balanced equation is as follows

\(2{H_2} + {O_2} \to 2{H_2}O\)

So, moles of H2

\(\begin{array}{l} = \frac{{{\rm{Given}}\,{\rm{mass}}}}{{{\rm{Molecular}}\,{\rm{weight}}}}\\ = \frac{{5g}}{{2g}}\\ = 2.5\,{\rm{moles}}\end{array}\)

So, moles of O2

\(\begin{array}{l} = \frac{{{\rm{Given}}\,{\rm{mass}}}}{{{\rm{Molecular}}\,{\rm{weight}}}}\\ = \frac{{10g}}{{32g}}\\ = 0.3125\,{\rm{moles}}\end{array}\)

02

Determine the limiting reactant

From the balanced equation, we can see that 2 mol of H2 produces 2 mol of H2O

So, 2.5 mol of H2 will produce = 2.5 x 2/2= 2.5 moles of H2O

1 mol of O2 produces 2 mol of H2O

0.1325 mol will produce = 0.3125 x 2 /1= 0.625 moles of H2O

As the amount of O2 is much smaller than H2. Hence the limiting reactant is O2.

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Most popular questions from this chapter

Colourful fireworks often involve the decomposition of barium nitrate and potassium chlorate and the reaction of metals magnesium, aluminium, and iron with oxygen.

(a)Write the formulae of barium nitrate and potassium chlorate.

(b)The decomposition of solid potassium chlorate leads to the formation of solid potassium chloride and diatomic oxygen gas. Write an equation for the reaction.

(c) The decomposition of solid barium nitrate leads to the formation of solid barium oxide, diatomic nitrogen gas and diatomic oxygen gas. Write an equation for the reaction.

(d)Write separate equations for the reactions of the solid metals magnesium, aluminium and iron and oxygen gas to yield the corresponding metal oxides.(Assume the iron oxide contains \(F{e^{3 + }}\)ions.)

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