Un método que se ha propuesto para eliminar el SO2 de los gases de combustión de las centrales t

Un método que se ha propuesto para eliminar el SO2 de los...

Un método que se ha propuesto para eliminar el $\mathrm{SO}_2$ de los gases de combustión de las centrales termoeléctricas incluye su reacción con $\mathrm{H}_2 \mathrm{~S}$ acuoso. El producto es azufre elemental. (a) Escriba una ecuación química balanceada de la reacción. (b) ¿Qué volumen de $\mathrm{H}_2 \mathrm{~S}$ a $27^{\circ} \mathrm{C}$ y 740 torr se necesitaria para eliminar el $\mathrm{SO}_2$ formado al quemar 1.0 ton de hulla que contiene $3.5 \%$ de S en masa? (c) ¿Qué masa de azufre elemental se produciría? Suponga que todas las reacciones alcanzan una eficiencia del $100 \%$.

Key Concepts

Balanced Chemical Equations

This concept involves writing and balancing chemical reactions so that the number of each type of atom is conserved between reactants and products. In chemical problem solving, balancing equations is the first crucial step that sets up the stoichiometric relationships necessary for further calculations.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows one to convert between masses, moles, and, in some cases, volumes of substances by using mole ratios derived from the balanced equation.

Percentage Composition

Percentage composition refers to the proportion by mass of a specific element within a compound or mixture. This is critical when determining how much of an element is present in a given mass of material, which is then converted to moles or other quantities in reaction calculations.

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates pressure, volume, temperature, and number of moles of a gas. This law is applied to determine the volume of gases under nonstandard conditions, facilitating calculations when gas reactants or products are involved.

Mole Concept

The mole concept is a fundamental chemical principle that uses the unit 'mole' to relate quantities of particles to mass. It underpins calculations that convert between the mass of substances and the number of moles, which is essential for applying stoichiometric relationships in chemical reactions.

Transcript

00:01 One method for removing sulfur dioxide from the flu gases of power plants involves reaction with aqueous hydrogen sulfide.

00:12 Elemental sulfur is the product.

00:14 Part a asks us to write the reaction.

00:19 And actually there are two.

00:22 So let's begin.

00:26 Each of these has a different form of hydrogen in them.

00:32 Just a sec to get back to my problem.

00:50 Okay, this equation is the equation i'm going to use for the rest of the calculations.

01:16 There's our first equation, and again, our second equation just has a different form of sulfur as a product.

01:53 Okay, so there's my two answers for part a.

02:03 Let's get ready for part b.

02:06 Part b.

02:10 What volume of h2s at 27 degrees celsius, which is 300 .15k, and 740 tor, which is 740 divided by 760? and i think that was, i wrote it down here.

02:42 Hang on, i closed my book by mistake.

02:50 737.

03:01 Okay, would we be required to remove the so2 that is formed by burning one ton of coal with 3 .5 % sulfur by mass? okay, let's start this by figuring out how much we have here.

04:01 So we have 2 ,000.

04:03 Pounds is a ton and we from a previous problem knew that there are 453 .6 grams per ton and we know that there's 32 .06 grams of sulfur per mole and we knew that this was 0 .0355 percent.

04:45 Let me punch the numbers into the calculator.

05:00 We get 990 .4.

05:12 Okay in s02 there's one s we've got a one -to -one relationship so that gives me 990 and now we can do our conversion our first conversion and if we look at our equations we can see that's a two and a one and then we'll multiply that by 22 .4 liters per mole in here let me verify this no, i didn't do it.

06:28 It's not at standard pressure, so i didn't do this...

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