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Chapter 22: Q22.50P (page 1019)

Why is commercial $H_{2} {SO}_{4}$ so inexpensive?

Short Answer

Expert verified

Since every step of the process is exothermic and heat is a useful by-product. So $H_{2} {SO}_{4}$ commercial is inexpensive.

Step by step solution

01

Concept Introduction

Sulfuric acid is created industrially by reacting water with sulphur trioxide which is made by combining sulphur dioxide and oxygen chemically using either the contact or chamber processes.

02

Information Provided

Every step of the process of production of $H_{2} {SO}_{4}$ is exothermic ((burning S, oxidizing ${SO}_{2}$ , hydrating ${SO}_{3}$ ), and heat is a desirable byproduct. The majority of the heat is sold as steam, with the remainder being used to circulate gases around the plant. A typical plant that produces 825 tonnes of $H_{2} {SO}_{4}$ per day generates enough steam to create ${7x10}^{6}$ watts of electricity.

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Most popular questions from this chapter

(a) What are the components of the reaction mixture following the water-gas shift reaction?

(b) Explain how zeolites (Gallery,) are used to purify the $H_{2}$ formed

The compounds ${({NH}_{4})}_{2} {HPO}_{4}$ and ${NH}_{4} (H_{2} {PO}_{4})$ are water-soluble fertilizers.

(a) Which has the higher mass $%$ of $P$ ?

(b) Why might the one with the lower mass $%$ of $P$ be preferred?

Describe two ways in which the biosphere has influenced the composition of Earth’s crust.

The lead(IV) oxide used in car batteries is prepared by coating the electrode plate with PbO and then oxidizing it to lead dioxide ( ${PbO}_{2}$ ). Despite its name, ${PbO}_{2}$ has a nonstoichiometric ratio of lead to oxygen of about. In fact, the holes in the ${PbO}_{2}$ crystal structure due to missing O atoms are responsible for the oxide’s conductivity. (a) What is the mole % of O missing from the ${PbO}_{2}$ structure? (b) What is the molar mass of the nonstoichiometric compound?

Question: Earth’s mass is estimated to be $5.98 \times 10^{24} kg$ , and titanium represents $0.05 %$ by mass of this total. (a) How many moles of are present? (b) If half of the $Ti$ is found as ilmenite $({FeTiO}_{3})$ , what mass of ilmenite is present? (c) If the airline and auto industries use $1.00 \times 10^{5}$ tons of $Ti$ per year, how many years would it take to use up all the $Ti (1 ton \times 2000 lb)$ ?

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