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Chapter 3: Q15DQ (page 83)

Question:One way of determining the empirical formula is to burn a compound in air and weigh theamounts of carbon dioxide and water given off. For what types of compounds does this work? Explain the assumptions that are made. Why is the formula an empirical formula and not necessarily a molecular formula?

Short Answer

Expert verified

Answer

Compounds which contains C, H and another kind of element.

Step by step solution

01

Work for hydrocarbons

Compounds which contains C, H and another kind of element. The compounds are CO₂ and H₂O can weight quantitatively.

02

Empirical and molecular formula

Both are not same. Because empirical formula denotes the simple whole number ratio for atoms in compound whereas molecular formula denotes the correct whole number ratio of atom in compound.

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Most popular questions from this chapter

Q.66. Iron oxide ores, commonly a mixture of FeO and Fe₂O₃are given the general formula Fe₃O₄.
They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes:

${Fe}_{3} O_{4} (s) + H_{2} (g) \to Fe (s) + H_{2} O (g) {Fe}_{3} O_{4} (s) + CO (g) \to Fe (s) + {CO}_{2} (g)$

Question:A sample of liquid heptane (C₇H₁₆) weighing 11.50 g is reacted with 1.300 moles of oxygen gas.The heptane is burned completely (heptane reacts with oxygen to form both carbon monoxideand water and carbon dioxide and water). After the reaction is complete, the amount of gaspresent is 1.050 moles (assume that all of the water formed is liquid).
a. How many moles of CO are produced?
b. How many moles of CO₂ are produced?
c. How many moles of O₂ are left over?

Nitric acid is produced commercially by the Ostwald process. The three steps of the Ostwaldprocess are shown in the following equations:
${4NH}_{3} (g) + 5 O_{2} (g) \to 4 NO (g) + 6 H_{2} O (g)$

$2 NO (g) + O_{2} (g) \to 2 {NO}_{2} (g)$

$3 {NO}_{2} (g) + H_{2} O (l) \to 2 {HNO}_{3} (a q) + NO (g)$

What mass of ${NH}_{3}$ must be used to produce $1.0 \times 10^{6} kg$ of ${HNO}_{3}$ by the Ostwald process, assumingyield in each reaction and assuming the $NO$ produced in the third stage is notrecycled?

Question:The percent by mass of nitrogen for a compound is found to be 46.7%. Which of the followingcould be this species?

A 0.755-g sample of hydrated copper(II) sulfate $(C_{u} {SO}_{4} \cdot {XH}_{2} O)$ was heated carefully until it had changed completely to anhydrous copper(II) sulfate $(C_{U} {SO}_{4})$ with a mass of 0.483 g. Determine the value of x. [This number is called the “number of waters of hydration" of copper(II) sulfate $(C_{U} {SO}_{4})$ . It specifies the number of water molecules per formula unit of in the hydrated crystal.]

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