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Chapter 3: 3.61P (page 133)

Reactants A and B form product C. Write a detailed Plan to find the mass of C when 25 g of A reacts with excess B.

Short Answer

Expert verified

In this case, as we know we have reactant B in excess which actually means that A is our limiting reactant.

Now calculate the moles of the limiting reactant.

Finally, with help of stoichiometry, we will get moles of that product.

Lastly, we multiply the moles with molecular mass and get the mass of C.

Step by step solution

01

Step1. Finding the limiting reactant.

In this case, as we know we have reactant B in excess which actually means that A is our limiting reactant.

Now calculate the moles of the limiting reactant.

Finally, with help of stoichiometry, we will get moles of that product.

Lastly, we multiply the moles with molecular mass and get the mass of C.

02

Step2. Final result

In this case, as we know we have reactant B in excess which actually means that A is our limiting reactant.

Now calculate the moles of the limiting reactant.

Finally, with help of stoichiometry, we will get moles of that product.

Lastly, we multiply the moles with molecular mass and get the mass of C.

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Most popular questions from this chapter

Cocaine (C17H21O4N) is a natural substance found in coca leaves, which have been used for centuries as a local anesthetic and stimulant. Illegal cocaine arrives in the United States either as the pure compound or as the hydrochloride salt (C17H21O4NHCl). At 25oC, the salt is very soluble in water (2.50 kg/L), but cocaine is much less so (1.70 g/L). (a) What is the maximum amount (in g) of the salt that can dissolve in 50.0 mL of water? (b) If the solution in part (a) is treated with NaOH, the salt is converted to cocaine. How much additional water (in L) is needed to dissolve it?

A 0.370 mol sample of a metal oxide (M203)weighs 55.4 g.
(a) How many moles of O are in the sample?
(b) How many grams of M are in the sample?
(c) What element is represented by the symbol M?

Many metals react with oxygen gas to form the metal oxide. For example, calcium reacts as follows:

2Ca(s)+O2(g)→2CaO(s)

You wish to calculate the mass of calcium oxide that can be prepared from 4.20 g of and 2.80 g of O2

(a) How many moles of CaO can be produced from the given mass of Ca ?

(b) How many moles of CaO can be produced from the given mass ofO2

(c) Which is the limiting reactant?

(d) How many grams of CaO can be produced?

For the reaction between solid tetraphosphorus trisulfide and oxygen gas to form solid tetraphosphorusdecaoxide and sulfur dioxide gas, write a balanced equation. Show the equation (see Table 3.5) in terms grams.

3.16 Calculate each of the following quantities:

(a) Mass in grams of 8.35 mol of copper(I) carbonate

(b) Mass in grams of4.04×1020 molecules of dinitrogen pentaoxide

(c) Number of moles and formula units in 78.9 g of sodium perchlorate

(d) Number of sodium ions, perchlorate ions, Cl atoms, and O atoms in the mass of the compound in part (c).
See all solutions

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