Consider the reaction: 2 SO2(g)+O2(g) ⟶2 SO3( s) (a) If...

Consider the reaction: $$ 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(\mathrm{~s}) $$ (a) If $285.5 \mathrm{~mL}$ of $\mathrm{SO}_{2}$ is allowed to react with $158.9 \mathrm{~mL}$ of $\mathrm{O}_{2}$ (both measured at STP), what is the limiting reactant and the theoretical yield of $\mathrm{SO}_{3} ?$ (b) If $2.805 \mathrm{~g}$ of $\mathrm{SO}_{3}$ is collected (measured at $\mathrm{STP}$ ), what is the percent yield for the reaction?

Consider the reaction:
$$
2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(\mathrm{~s})
$$
(a) If $285.5 \mathrm{~mL}$ of $\mathrm{SO}_{2}$ is allowed to react with $158.9 \mathrm{~mL}$ of $\mathrm{O}_{2}$ (both measured at STP), what is the limiting reactant and the theoretical yield of $\mathrm{SO}_{3} ?$
(b) If $2.805 \mathrm{~g}$ of $\mathrm{SO}_{3}$ is collected (measured at $\mathrm{STP}$ ), what is the percent yield for the reaction?

Key Concepts

Balanced Chemical Equations

Balanced chemical equations provide the foundation for quantitative analysis in chemical reactions. They show the exact proportions in which reactants combine and products form, based on the law of conservation of mass. This concept allows for the use of stoichiometric coefficients to calculate how much of each substance is required or produced in a reaction.

Stoichiometry

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. It uses the mole ratios derived from the balanced equation to convert between amounts, such as mass or volume at a given condition, which is essential for determining quantities like theoretical yields and identifying limiting reactants.

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is completely consumed first, thus limiting the amount of product that can be formed. Identifying the limiting reactant is crucial in stoichiometric calculations because it determines the maximum theoretical amount of product that can be produced from the given reactants.

Theoretical Yield

The theoretical yield refers to the maximum amount of product that can be produced in a chemical reaction, as predicted by stoichiometry, under the assumption that the reaction proceeds perfectly with no losses. It is calculated based on the limiting reactant and the stoichiometric ratios from the balanced chemical equation.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction. It is calculated by dividing the actual yield (the amount of product actually obtained from the reaction) by the theoretical yield, then multiplying by 100. This concept helps in assessing the performance of a reaction, taking into account practical limitations and losses.

Mole Concept

The mole concept is a fundamental principle in chemistry that provides a bridge between the atomic scale and the macroscopic scale. It allows chemists to count entities such as atoms, molecules, or ions in a given mass or volume by using Avogadro's number, facilitating conversions in stoichiometry and helping to quantify substances in a reaction.

Standard Temperature and Pressure (STP)

Standard Temperature and Pressure (STP) refers to a set of standard conditions for experimental measurements, typically 0°C (273.15 K) and 1 atm pressure. Under STP, one mole of any ideal gas occupies 22.4 liters, which significantly simplifies calculations involving gases, as volume ratios can be directly related to mole ratios in reactions involving gaseous reactants or products.

Transcript

0:00 Hi everyone.

00:01 So first will date given data, you know volume of assertive they are given and that is equal to 285 .5 m.

00:19 So this you have to convert into liter by dividing by 1000s.

00:24 So 0 .285 liter then volume of 4 -2 they provided of course this is a part volume of o2 158 .9 ml that is equal to 0 .1589 litre.

00:59 What is the limiting reactant? secondly, they ask theoretical yield of so3, theoretical yield of so3, so3, and in p.

01:35 And in p.

01:37 They provided us volume of so3 weight of so3 that is 2 .805 gram so first of of all right the reaction you know twice so2 gas plus o2 gas gas gas twice so3 gas now first you have to calculate number of moles of acid that is equal to pv upon rt.

02:23 This is from general gas equation.

02:25 Pv is equal to nrt and that's why again is equal to pv upon r2.

02:32 You know, they mention a hpp.

02:35 So pressure at http is one even we'll mention this in the given data that is pressure at http is 1 atmosphere and temperature is 273 .15 kelvin.

02:57 So this is 1 into volume of so2.

03:08 .2855 divided by r0 .082 into temperature 273 .15.

03:20 So that is equal to 0 .082 into temperature 2855 divided by 22 .3983.

03:41 Therefore, n of s.

03:43 That is equal to 0 .012765 moles.

04:04 So these are moles of s .o2.

04:10 Then second step is to calculate moles of o2 and of o2 and that is equal to a pv upon r3.

04:25 That is equal to pressure is 1.

04:28 Then volume is 01589 divided by r 0 .082 into 273 .15...