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(a)
Interpretation:
To calculate the mass of
Concept introduction:
Ammonium perchlorate upon decomposition gives
The total number of moles of the substance is equal to the mass of the substance divided by the molecular weight of that substance.
The limiting reagent in the
(a)
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Answer to Problem 98GQ
The mass of water molecule is produced upon decomposition of ammonium perchlorate is
The mass of oxygen molecule is produced upon decomposition of ammonium perchlorate is
Explanation of Solution
The mass of
Given:
The mass of ammonium perchlorate is
The balanced chemical equation of decomposition of ammonium perchlorate is written as,
The number of moles
From equation (1), two moles of ammonium perchlorate produced four moles of water molecules. Therefore, the number of moles
The mass
Therefore, the mass of water molecule is produced upon decomposition of ammonium perchlorate is
From equation (1), two moles of ammonium perchlorate produced one mole of the oxygen molecule. Therefore, the number of moles
The mass
Therefore, the mass of oxygen molecule is produced upon decomposition of ammonium perchlorate is
(b)
Interpretation:
To calculate the mass of aluminium which is required to use up all of the oxygen to form
Concept introduction:
Ammonium perchlorate upon decomposition gives
The total number of moles of the substance is equal to the mass of the substance divided by the molecular weight of that substance.
The limiting reagent in the chemical reaction is the substance that is totally consumed when the chemical reaction is complete. The amount of product formed is limited by the limiting reagent.
(b)
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Answer to Problem 98GQ
The mass of aluminium powder which is required to use up all of the oxygen to form
Explanation of Solution
The mass of aluminium which is required to use up all of the oxygen to form
Given:
The number of moles of oxygen molecule calculated in sub-part (a) is
The balanced chemical equation of the reaction of aluminium with oxygen molecule is written as,
Since the entire oxygen molecule is used to react with the aluminium powder to produce
From equation (2), four moles of aluminium reacted with three moles of the oxygen molecule. Therefore, the number of moles
The mass
Therefore, the mass of aluminium powder which is required to use up all of the oxygen to form
(c)
Interpretation:
To calculate the mass of
Concept introduction:
Ammonium perchlorate upon decomposition gives
The total number of moles of the substance is equal to the mass of the substance divided by the molecular weight of that substance.
The limiting reagent in the chemical reaction is the substance that is totally consumed when the chemical reaction is complete. The amount of product formed is limited by the limiting reagent.
(c)
![Check Mark](/static/check-mark.png)
Answer to Problem 98GQ
The mass of
Explanation of Solution
The mass of
Given:
The mass of aluminium powder which is required to use up all of the oxygen to form
The balanced chemical equation of the reaction of aluminium with oxygen molecule is written as,
Four moles of aluminium produced two moles of
The mass
Therefore, the mass of
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Chapter 21 Solutions
Chemistry & Chemical Reactivity
- 4.48 Elemental phosphorous is used in the semiconductor industry. It can be obtained from an ore called fluoroapatite via reaction with SiO2 and C: 4Ca5( PO4)3F+18SiO2+30C3P4+30CO+18CaSiO3+2CaF2 Suppose a particular semiconductor production plant requires 1500 kg of P4. If the recovery of P4 from this reaction is 73% efficient, what mass of fluoroapatite is needed?arrow_forwardWhat is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of mercury, if the fish contains 30 parts per million of mercury by weight? (Assume that all the mercury from the fish ends up as mercury (II) chloride in the body and that a fatal dose is 0.20 g of HgCl2.) How many pounds of fish is this?arrow_forward4.22 Generally, an excess of O2 is needed for the reaction Sn+O2SnO2 . What is the minimum number of moles of oxygen required to oxidize 7.3 moles of tin?arrow_forward
- Complete and balance the equations of the following reactions, each of which could be used to remove hydrogen sulfide from natural gas: (a) Ca(OH)2(s)+H2S(g) (b) Na2CO3(aq)+H2S(g)arrow_forwardPhosphoric acid, H3PO4, can be prepared by the reaction of phosphorus(V) oxide, P4O10, with water. 14P4O10(s)+32H2O(l)H3PO4(aq);H=96.2kJ What is H for the reaction involving 1 mol of P4O10? P4O10(s)+6H2O(l)4H3PO4(aq)arrow_forwardWrite balanced equations for the reaction of scandium metal to produce the scandium(III) salt with the following nonmetals: (a) sulfur (c) nitrogen (b) chlorine (d) oxygen (forming the oxide)arrow_forward
- The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3Al(s)+3NH4ClO4(s)Al2O3(s)+AlCl3(s)+3NO(g)+6H2O(g) Calculate H for this reactionarrow_forwardWrite balanced chemical equations for the following reactions: (a) metallic aluminum burned in air (b) elemental aluminum heated in an atmosphere of Chlorine (c) aluminum heated in hydrogen bromide gas (d) aluminum hydroxide added to a solution of nitric acidarrow_forwardNitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.arrow_forward
- Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?arrow_forwardThe carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardChlorine exists mainly as two isotopes, 37Cl and 33Cl. Which is more abundant? How do you know?arrow_forward
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