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Chapter 3: Problem 117

Which of the following has the greater mass: \(0.72 \mathrm{~g}\) of \(\mathrm{O}_{2}\) or 0.0011 mole of chlorophyll \(\left(\mathrm{C}_{55} \mathrm{H}_{72} \mathrm{MgN}_{4} \mathrm{O}_{5}\right) ?\)

Short Answer

Expert verified
The substance with the greater mass between the calculated mass of chlorophyll and the given mass of \(O_2\) is [fill in upon computation]

Step by step solution

01

Determine the molecular weights

Calculate the molecular weight of \(O_2\) and chlorophyll. The molecular weight of an oxygen molecule (\(O_2\)) is \(2 \times 16 = 32 \mathrm{~g/mol}\). For chlorophyll, \(C_{55} H_{72} MgN_{4} O_{5}\), we add up the atomic masses of all the atoms to determine the molecular weight:\[55 \times \mathrm{Mass~of~C} + 72 \times \mathrm{Mass~of~H} + \mathrm{Mass~of~Mg} + 4 \times \mathrm{Mass~of~N} + 5 \times \mathrm{Mass~of~O}\]
02

Calculate the mass of chlorophyll

Using the molecular weight of chlorophyll and the given amount in moles, calculate the mass. Mass is calculated by multiplying the number of moles by the molecular weight. Thus, the mass of chlorophyll is \((\mathrm{Moles~of~chlorophyll}) \times (\mathrm{Molecular Weight~of~chlorophyll})\).
03

Compare the masses

This step involves comparing the given mass of \(O_2\) (0.72 g) with the calculated mass of chlorophyll from Step 2. The substance with the greater mass is the answer to the exercise.

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Most popular questions from this chapter

Write balanced equations for the following reactions described in words. (a) Pentane burns in oxygen to form carbon dioxide and water. (b) Sodium bicarbonate reacts with hydrochloric acid to form carbon dioxide, sodium chloride, and water. (c) When heated in an atmosphere of nitrogen, lithium forms lithium nitride. (d) Phosphorus trichloride reacts with water to form phosphorus acid and hydrogen chloride. (e) Copper(II) oxide heated with ammonia will form copper, nitrogen gas, and water.

A certain metal M forms a bromide containing 53.79 percent Br by mass. What is the chemical formula of the compound?

The annual production of sulfur dioxide from burning coal and fossil fuels, auto exhaust, and other sources is about 26 million tons. The equation for the reaction is$$\mathrm{S}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g)$$How much sulfur (in tons), present in the original materials, would result in that quantity of \(\mathrm{SO}_{2} ?\)

An iron bar weighed \(664 \mathrm{~g}\). After the bar had been standing in moist air for a month, exactly one-eighth of the iron turned to rust \(\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right) .\) Calculate the final mass of the iron bar and rust.

Why must a chemical equation be balanced? What law is obeyed by a balanced chemical equation?
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