What is the percent yield of a reaction in which 45.5 g of tungsten(VI) oxide (WO3) reacts with

What is the percent yield of a reaction in which 45.5 g of...

Key Concepts

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield (the amount of product actually obtained from the experiment) to the theoretical yield (the amount of product predicted by stoichiometric calculations based on complete conversion of the limiting reactant). This concept is fundamental in assessing how well a reaction proceeds under given conditions.

Molar Mass and Conversion

Understanding and calculating the molar mass of substances is crucial because it allows conversion between mass and moles, the unit used in stoichiometric calculations. This conversion is essential when working with chemical equations to quantify reactants and products.

Stoichiometry

Stoichiometry involves using coefficients in a balanced chemical equation to determine the relationships and ratios between reactants and products. It provides a systematic method to predict yields and to calculate the amounts of substances consumed or produced in a chemical reaction.

Density and Mass-Volume Relationship

The relationship between density, mass, and volume is used to interconvert these quantities when one of them is provided. In reactions where the product is a liquid, knowing its density allows the determination of its mass from its volume, which can then be converted to moles for further stoichiometric analysis.

Transcript

00:01 So what will be the percentage yield? if we have a constant for oxide, we have with excess hydrogen, the proteose, metalin tons and also 9 .6 militer of water.

00:13 Okay, so first of all, we have 45 .5 gram of tungsten for oxide, and then we have water, and two be podules, and also with the methane tungsten.

00:25 We have to first balance the chemical reaction, because we have to do it in order to, have a proper circuitometry and motor ratio between reactants.

00:36 So i will put a fluid in front of water in order to keep our tendons for oxide to be one.

00:43 So i already balanced tungsten and also oxygen.

00:48 So the last thing that i'm going to balance would be our hydrogen.

00:53 Okay, so we have a balanced chemical reaction.

00:58 And then for hydrogen in excess, so you already know that, and we have to find the percentage yield.

01:05 So for percentage yield, it's equal to the mass that we actually, of the product, we actually measure.

01:15 So experimental value is it experimental.

01:21 We actually do experimental file, all far off the, again, the mass of the product, but it will be, theoretical, theoretical.

01:32 So you just assume everything we add 100 % is good and then time 100%.

01:38 Okay, so we have to find the mass of pot that that is experimental.

01:42 And also we have to find the mass of the pot that that is theoretical.

01:47 Okay, so first of all for the mass of the pot that is experimental, it's pretty straightforward to find out because we can just look at the amount of water produce.

01:56 So the amount of water produce is 9 .6 millilitre, and then that that is 1 gram per meter.

02:02 So we can conclude that the mass of the power that we can look at water, it will be equals to 9 .60 gram from the actual experiment that measure.

02:14 So we have to find out the theoretical mass of water produced if we have all of the tendons for oxides being reacted.

02:24 Okay, so we have to complete this equation, but let's find out the figure of mass.

02:29 Okay, first of four, we have 45 .5 gram of tons and four oxide.

02:35 We have to convert that to lumbermoremoremore most.

02:37 So first of first of all, let's file the molar mass of tonson for oxide.

02:41 So we are 183 .9 for the motor mass of tungsten plus 16 times three...

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