Question

4. (5) How many moles of carbon monoxide can be made from a mixture of 9.15 mol Fe(CO)5, 11.23 mol PF3 and 8.76 mol H2? (think ratios, must show all calculations) Fe(CO)5 (0) + 2PF3 (g) + H2 (g) \rightarrow Fe(CO)2(PF3)2H2(g) + 3 CO (g) 5. (6) What mass of silver is required to completely react with 18.59 g of oxygen, according to the unbalanced equation below? Ag (s) + O2 (g) \rightarrow Ag2O (s) 6. (6) How many grams of CO2 will be produced when 54.85 g of pentane reacts with an excess of oxygen, according to the unbalanced chemical reaction below: C5H12 (l) + O2 (g) \rightarrow CO2 (g) + __ H2O (g)

          4. (5) How many moles of carbon monoxide can be made from a mixture of 9.15 mol
Fe(CO)5, 11.23 mol PF3 and 8.76 mol H2? (think ratios, must show all calculations)
Fe(CO)5 (0) + 2PF3 (g) + H2 (g) \rightarrow Fe(CO)2(PF3)2H2(g) + 3 CO (g)
5. (6) What mass of silver is required to completely react with 18.59 g of oxygen,
according to the unbalanced equation below?
__ Ag (s) + __ O2 (g) \rightarrow __ Ag2O (s)
6. (6) How many grams of CO2 will be produced when 54.85 g of pentane reacts with an
excess of oxygen, according to the unbalanced chemical reaction below:
__ C5H12 (l) + __ O2 (g) \rightarrow __ CO2 (g) + __ H2O (g)

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4. (5) How many moles of carbon monoxide can be made from a mixture of 9.15 mol
Fe(CO)5, 11.23 mol PF3 and 8.76 mol H2? (think ratios, must show all calculations)
Fe(CO)5 (0) + 2PF3 (g) + H2 (g) →Fe(CO)2(PF3)2H2(g) + 3 CO (g)
5. (6) What mass of silver is required to completely react with 18.59 g of oxygen,
according to the unbalanced equation below?
Ag (s) + O2 (g) →Ag2O (s)
6. (6) How many grams of CO2 will be produced when 54.85 g of pentane reacts with an
excess of oxygen, according to the unbalanced chemical reaction below:
C5H12 (l) + O2 (g) →CO2 (g) + H2O (g)

Added by Brooke T.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Jennifer Hudspeth

06/16/2022

Step 1

Fe(CO)5(m) + 2PF3(g) + H2(g) > Fe(CO)2(PF3)2H2(g) + 3CO(g) Show more…

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4.(5) How many moles of carbon monoxide can be made from a mixture of 9.15 mol Fe(CO)s, 11.23 mol PF3 and 8.76 mol H2? (think ratios,must show all calculations Fe(CO)5(m)+2PF3(g)+ H2(g)> Fe(CO)2(PF3)2H2(g +3 CO(g) 5.(6 What mass of silver is required to completely react with 18.59 g of oxygen according to the unbalanced equation below? Ag (s)+ O2(g) Ag2O (s) 6. (6) How many grams of CO2 will be produced when 54.85 g of pentane reacts with an excess of oxygen, according to the unbalanced chemical reaction below: CsH(+ O2 (g) > CO+ HO

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Transcript

00:02 Hi there.

00:03 In this question, we are given this balanced equation, and we are told that we are burning 19 .8 grams of the c5h12 of the pentate.

00:16 And we want to know how many grams of carbon dioxide can be produced.

00:20 What is the mass? so question mark grams.

00:25 All right.

00:25 Well, to convert from one substance to another in a chemical equation, we need to use the mole ratio.

00:30 So because this is a mass to mass stoichiometry problem.

00:35 So in order to convert from one substance to the other, we need that mole ratio.

00:40 And the mole ratio is found by using the coefficients in the balanced equation.

00:44 Since nothing is written in front of the pentane, it's understood that it's a one.

00:48 So for every one mole of pentane, we can produce five moles of carbon dioxide.

00:54 However, right now we do not have moles.

00:57 So our first step is going to be to convert from grams of the pentane to moles.

01:03 And we'll that by using the molar mass given to us in the problem.

01:08 Then we can use that 1 to 5 mole ratio to convert to moles of carbon dioxide.

01:15 And then finally we can convert from moles of carbon dioxide to mass by using carbon dioxide's molar mass, which is also given to us in the problem.

01:28 All right.

01:29 So this is our plan.

01:30 It's going to take us three steps to get from our starting point of 19 .8 grams of c5, h12...

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