Using the models of the molecules (black = C, white = H, yellow =...

Question

Using the models of the molecules (black = C, white = H, yellow = S, red = O) determine each of the following for models of compounds 1 and 2: (7.1,7.2, 7.3)1.

3D models of molecules showing carbon, hydrogen, sulfur, and oxygen atoms for chemistry exercises.

2.

c. number of moles in 10.0 g

Accepted Answer

Hey, everyone, we're asked to consider the molecular model shown in the figure below where gray is carbon white is hydrogen, red is oxygen blue, is nitrogen, yellow, green is fluorine. We're asked to determine the number of moles for compound one and compound two. If each has a mass of 28.0 g, starting with compound one, we can see that we have one gray, which means we have one carbon. Next, we have one red, which means we have one oxygen. Next, we can see that we have two yellow green, which means we have two of fluorine. Now, when we put these all together, we end up with a formula of C O F two, which is the formula for carbonyl fluoride. Next, let's go ahead and take a look at compound two for compound two. We can see that we have 12344 of our gray, which means that we have four of carbon. Next, looking at our white, we have 1234 and five, we have five of white, which means we have five of hydrogen. And lastly looking at our blue, we have one of blue, which means we have one of nitrogen, putting this all together our molecular formula comes up to C 4h five N, which is the formula for peril. Now that we have our formulas, let's go ahead and determine the number of moles for compound one and two, Starting with our compound one. We first need to determine our molar mass for our carbonyl fluoride. Starting with our carbon. We have one of carbon and we're going to multiply this by its atomic mass of 12.01 g per mole. Next, we're going to add in our oxygen and we have one of oxygen and we're going to multiply this by its atomic mass of 16.00 g per mole. Next, looking at our fluorine, we have two of fluorine and we're going to multiply this by its atomic mass of 19.00 g per mole. So when we calculate this out, we end up with a molar mass of 66.01 g per mole of our carbonyl fluoride. Now to determine our moles of carbonyl fluoride, we're going to take 28.0 g of carbonyl fluoride, which was provided to us in our question stem and we're going to use dimensional analysis here. So we calculated that we had 66.1 g of carbonyl fluoride per one mole of carbonyl fluoride. So when we calculate this out and cancel out our units, we end up with 0.424 mole of carbonyl fluoride, which is going to be one of our answers for this question. Now, let's go ahead and move on to compound two, our payroll again, we're going to take our molar mass of pure Starting with our carbon. We can see that we have four of carbon and we're going to multiply this by its atomic mass of 12.01 g per mole. Next, adding in our hydrogen, we have five of hydrogen and we're going to multiply this by its atomic mass of 1.008 g per mole. Next, looking at our nitrogen, we have one of nitrogen and we're going to multiply this by its atomic mass of 14.01 g per mole. Now when we calculate this out, we end up with a molar mass of 67.09 g per mole. Now let's go ahead and use this value to determine our moles of peril Again, starting with 28.0 g of pure. We're going to use our molar mass for our dimensional analysis and we know that we have 67.09 g of pal per one mole of peril. So when we calculate this out and cancel out all of our units, We end up with 0.417 mole of peril and this is going to be our other final answer. Now, I hope this made sense and let us know if you have any questions.

Using the models of the molecules (black = C, white = H, yellow = S, red = O) determine each of the following for models of compounds 1 and 2: (7.1,7.2, 7.3)1.
2.
c. number of moles in 10.0 g

TextbookSolutions.keyConceptsTitle

Molecular Composition

Moles and Molar Mass

Stoichiometry

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