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Outline the steps needed to determine the limiting reactant when 0.50 mol of Cr and 0.75 mol of H3PO4 react according to the following chemical equation.\(2Cr + 2{H_3}P{O_4} \to 2CrP{O_4} + 3{H_2}\). Determine the limiting reactant.

Short Answer

Expert verified

Cr is the limiting reactant.

Step by step solution

01

Determine the number of moles

Find the number of moles of \({H_3}P{O_4}\).

Mol\({H_3}P{O_4} = 0.50\,mol\,Cr\,\left( {\frac{{2\,mol\,{H_3}P{O_4}}}{{2\,mol\,Cr}}} \right) = 0.50\,mol\,{H_3}P{O_4}\).

02

Determine the limiting reactant

Only 0.50 mol of\({H_3}P{O_4}\)is required but we have 0.75 mol of\({H_3}P{O_4}\)so, \({H_3}P{O_4}\)is in excess amount. Thus, Cr is the limiting reactant.

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Most popular questions from this chapter

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.

2Clโˆ’(aq) + Hg(NO3)2(aq)โŸถ2NO3โˆ’(aq) + HgCl2(s)

What is the Clโˆ’ concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of 8.25ร—10โˆ’4MHg(NO3)2(aq) to reach the end point?

How many NH3 molecules are produced by the reaction of 4 mol of Ca(OH)2 according to the following reaction

\({\left( {N{H_4}} \right)_2}S{O_4} + Ca{\left( {OH} \right)_2} \to 2N{H_3} + CaS{O_4} + 2{H_2}O\)

Complete and balance each of the following oxidation-reduction reactions, such that it results in the highest possible oxidation states for the oxidizing atoms:

(a)\(K\left( s \right) + {H_2}O\left( l \right) \to \)

(b)\(Ba\left( s \right) + HBr\left( {aq} \right) \to \)

(c) \(Sn\left( s \right) + {I_2}\left( s \right) \to \)

Use the following equations to answer the next four questions:

i.\({H_2}O\left( s \right) \to {H_2}O\left( l \right)\)

ii.\(N{a^ + }\left( {aq} \right) + C{l^ - }\left( {aq} \right) + A{g^ + }\left( {aq} \right) + NO_3^ - \left( {aq} \right) \to AgCl\left( s \right) + N{a^ + }\left( {aq} \right) + NO_3^ - \left( {aq} \right)\)

iii.\(C{H_3}OH\left( g \right) + {O_2}\left( g \right) \to C{O_2}\left( g \right) + {H_2}O\left( g \right)\)

iv. \(2{H_2}O\left( l \right) \to 2{H_2}\left( g \right) + {O_2}\left( g \right)\)

v. \({H^ + }\left( {aq} \right) + O{H^ - }\left( {aq} \right) \to {H_2}O\left( l \right)\)

(a) Which equation describes a physical change?

(b)Which equation identifies the reactants and products of a combustion reaction?

(c)Which equation is not balanced?

(d)Which is a net ionic equation?

Write a balanced molecular equation describing each of the following chemical reactions.

(a) Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas

(b)Gaseous butane reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor

(c)Aqueous solution of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride

(d) Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.

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