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Chapter 4: Q70E (page 173)

Outline the steps needed to determine the limiting reactant when 30.0 g of propane,\({C_3}{H_8}\), is burned with 75.0 g of oxygen. Determine the limiting reactant.

Short Answer

Expert verified

Steps for limiting reactant.

  1. Write the balanced chemical equation.
  2. Find the molar mass of propane\({C_3}{H_8}\)and\({O_2}\).
  3. Find the mass of \({O_2}\) required to burn 30.0g \({C_3}{H_8}\).
  4. If the mass of \({O_2}\) present is more, \({O_2}\) is in excess. Hence, \({C_3}{H_8}\) is the limited reactant. If not, the \({O_2}\) is the limited reactant.

Step by step solution

01

Balanced chemical equation

Write the combustion of propane as

\(\)\(\)\({C_3}{H_8} + {O_2} \to C{O_2} + {H_2}O\)

Balance the equation by putting coefficients.

\({C_3}{H_8} + 5{O_2} \to 3C{O_2} + 4{H_2}O\)

02

Determine molar mass

\(\begin{aligned}{}1\,mol\,{C_3}{H_8} = 3\left( {12.011} \right) + 8\left( {1.008} \right)\\ = 44.097g\\1\,mol\,{O_2} = 2\left( {15.999} \right)\\ = 31.998g\end{aligned}\).

03

Determine mass of O2 required

Find the mass of \({O_2}\)required to burn 30.0g propane.

\(\begin{aligned}{}30.0\,g\,{C_3}{H_8}\left( {\frac{{1\,\,mol\,{C_3}{H_8}}}{{44.097\,g\,{C_3}{H_8}}}} \right)\left( {\frac{{5\,mol\,{O_2}}}{{1\,mol\,{C_3}{H_8}}}} \right)\left( {\frac{{31.998\,g\,{O_2}}}{{1\,mol\,{O_2}}}} \right) = 109\,g\,{O_2}\\75.0\,g{O_2} < 109\,g\,{O_2}\end{aligned}\)

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Most popular questions from this chapter

The balanced molecular equations, write the complete ionic and net ionic equations for the following

(a)\({K_2}{C_2}{O_4}\left( {aq} \right) + Ba{\left( {OH} \right)_2}\left( {aq} \right) \to 2KOH\left( {aq} \right) + B{a_2}{C_2}{O_4}\)

(b)\(Pb{\left( {N{O_3}} \right)_2}\left( {aq} \right) + {H_2}S{O_4}\left( {aq} \right) \to PbS{O_4} + 2HN{O_3}\)

(c)\(CaC{O_3}\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to CaS{O_4} + C{O_2} + {H_2}O\)

What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503MAgNO3 requires 20.22 mL of the AgNO3 solution to reach the end point?

AgNO3(aq) + NaCl(aq)⟶AgCl(s) + NaNO3(aq)

In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO3)2 solution.

2Cl−(aq) + Hg(NO3)2(aq)⟶2NO3−(aq) + HgCl2(s)

What is the Cl− concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of 8.25×10−4MHg(NO3)2(aq) to reach the end point?

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.)

A sample of solid calcium hydroxide, Ca(OH)2is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00×10-2M HCl requires 36.6 mL of the acid to reach the end point.

\({\rm{Ca(OH}}{{\rm{)}}_{2({\rm{aq}})}}{\rm{ + 2HC}}{{\rm{l}}_{({\rm{aq}})}}{\rm{ }} \to {\rm{ CaC}}{{\rm{l}}_{2({\rm{aq}})}}{\rm{ + 2}}{{\rm{H}}_2}{{\rm{O}}_{({\rm{l}})}}\)

What is the molarity?
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