Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 50

Liquid ethyl mercaptan, \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{S},\) has a density of \(0.84 \mathrm{g} / \mathrm{mL} .\) Assuming that the combustion of this compound produces only \(\mathrm{CO}_{2}, \mathrm{H}_{2} \mathrm{O},\) and \(\mathrm{SO}_{2},\) what masses of each of these three products would be produced in the combustion of \(3.15 \mathrm{mL}\) of ethyl mercaptan?

Short Answer

Expert verified
The masses of each combustion product are: \(CO_{2}: 3.74 \, \mathrm{g}\), \(H_{2}O: 2.30 \, \mathrm{g}\), \(SO_{2}: 2.72 \, \mathrm{g}\)

Step by step solution

01

Balance the chemical equation

First, we write down the unbalanced chemical equation: \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{S} + \mathrm{O}_2 \rightarrow \mathrm{CO}_{2} + \mathrm{H}_{2} \mathrm{O} + \mathrm{SO}_{2}\). We then balance this equation: \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{S} + 5 \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_{2} + 3 \mathrm{H}_{2} \mathrm{O} + \mathrm{SO}_{2 }\)
02

Find the molar mass of ethyl mercaptan

Using the periodic table, we determine the molar masses of each atom and sum them together to find the molar mass of ethyl mercaptan. Ethyl mercaptan \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{S}\) has a molar mass of \((2*12.01) + (6*1.008) + 32.07 = 62.146 \, \mathrm{g/mol} \)
03

Convert volume to mass to moles

We know that the density is the mass divided by the volume i.e., \(density = \frac{mass}{volume}\). We can solve this for mass and substitute the given volume and density into this equation. We therefore have: \(mass = 0.84 \, \mathrm{g/mL} * 3.15 \, \mathrm{mL} = 2.646 \, \mathrm{g}\). Then, we convert this mass to moles using the molar mass from step 2 i.e., \(moles = \frac{mass}{molar \, mass} = \frac{2.646 \, \mathrm{g}}{62.146 \, \mathrm{g/mol}} = 0.0425 \, \mathrm{mol}\)
04

Use stoichiometry to find amounts of products

From the balanced chemical equation, we know that each mol of ethyl mercaptan (\(C_{2}H_{6}S\)) produces 2 mol of carbon dioxide (\(CO_{2}\)), 3 mol of water (\(H_{2}O\)) and 1 mol of sulfur dioxide (\(SO_{2}\)). So, we calculate the amounts of each product respectively: \(0.0425 \, \mathrm{mol} * 2 = 0.0850 \, \mathrm{mol} \, CO_{2}\), \(0.0425 \, \mathrm{mol} * 3 = 0.1275 \, \mathrm{mol} \, H_{2}O\), and \(0.0425 \, \mathrm{mol} * 1 = 0.0425 \, \mathrm{mol} \, SO_{2}\)
05

Convert moles of products to gram

Using the molar masses of each compound (\(CO_{2}: 44.01 \, \mathrm{g/mol}\), \(H_{2}O: 18.02 \, \mathrm{g/mol}\), \(SO_{2}: 64.07 \, \mathrm{g/mol}\)), we calculate the mass of each product: \(0.0850 \, \mathrm{mol} \, CO_{2} * 44.01 \, \mathrm{g/mol} = 3.74 \, \mathrm{g} \, CO_{2}\), \(0.1275 \, \mathrm{mol} \, H_{2}O * 18.02 \, \mathrm{g/mol} = 2.30 \, \mathrm{g} \, H_{2}O\), and \(0.0425 \, \mathrm{mol} \, SO_{2} * 64.07 \, \mathrm{g/mol} = 2.72 \, \mathrm{g} \, SO_{2}\). These are the masses of each combustion product.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Determine the mass percent \(O\) in the mineral malachite, \(\mathrm{Cu}_{2}(\mathrm{OH})_{2} \mathrm{CO}_{3}\)

Which answer is correct? One mole of liquid bromine, \(\mathrm{Br}_{2},\) (a) has a mass of \(79.9 \mathrm{g} ;\) (b) contains \(6.022 \times 10^{23}\) Br atoms; (c) contains the same number of atoms as in \(12.01 \mathrm{g} \mathrm{H}_{2} \mathrm{O} ;\) (d) has twice the mass of 0.500 mole of gaseous \(\mathrm{Cl}_{2}\)

Supply the formula for the acids: (a) hydrofluoric acid; (b) nitric acid; (c) phosphorous acid; (d) sulfuric acid.

Assign suitable names to the compounds (a) \(\mathrm{CS}_{2}\) (b) \(\operatorname{SiF}_{4} ;\) (c) \(\operatorname{ClF}_{5} ;\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5} ;\) (e) \(\mathrm{SF}_{6} ;\) (f) \(\mathrm{I}_{2} \mathrm{Cl}_{6}\).

Three of the following formulas might be either an empirical or a molecular formula. The formula that must be a molecular formula is (a) \(\mathrm{N}_{2} \mathrm{O} ;\) (b) \(\mathrm{N}_{2} \mathrm{H}_{4}\) (c) \(\mathrm{NaCl} ;\) (d) \(\mathrm{NH}_{3}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free