Question

14. What volume of benzene (C6H6) is required to produce 1.5 x 10³ kJ of energy according the reaction below? The density of benzene is 0.88 g/mL. 2 C6H6 (l) + 15 O2 (g) ? 12 CO2 (g) + 6 H2O (g) ?E = -6278 kJ (a) 75 mL (b) 37 mL (c) 21 mL (d) 19 mL (e) 42 mL 15. Suppose the following reaction is performed in a perfect coffee cup calorimeter using 1.22 g of magnesium metal, 100.0 g of water, and 22.0 g HCl. The reaction solution has a specific heat of 4.184 J/g °C. Mg (s) + 2 HCl (aq) ? MgCl2 (aq) + H2 (g)

          14. What volume of benzene (C6H6) is required to produce 1.5 x 10³ kJ of energy according the reaction below? The density of benzene is 0.88 g/mL.

2 C6H6 (l) + 15 O2 (g) ? 12 CO2 (g) + 6 H2O (g) ?E = -6278 kJ

(a) 75 mL
(b) 37 mL
(c) 21 mL
(d) 19 mL
(e) 42 mL

15. Suppose the following reaction is performed in a perfect coffee cup calorimeter using 1.22 g of magnesium metal, 100.0 g of water, and 22.0 g HCl. The reaction solution has a specific heat of 4.184 J/g °C.

Mg (s) + 2 HCl (aq) ? MgCl2 (aq) + H2 (g)

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14. What volume of benzene (C6H6) is required to produce 1.5 x 10³ kJ of energy according the reaction below? The density of benzene is 0.88 g/mL.

2 C6H6 (l) + 15 O2 (g) ? 12 CO2 (g) + 6 H2O (g) ?E = -6278 kJ

(a) 75 mL
(b) 37 mL
(c) 21 mL
(d) 19 mL
(e) 42 mL

15. Suppose the following reaction is performed in a perfect coffee cup calorimeter using 1.22 g of magnesium metal, 100.0 g of water, and 22.0 g HCl. The reaction solution has a specific heat of 4.184 J/g °C.

Mg (s) + 2 HCl (aq) ? MgCl2 (aq) + H2 (g)

Added by Marissa P.

Chemistry

Paul Flowers, Klaus Theopold, Richard…

Chapter 15

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Solved by Expert Jennifer Hudspeth

04/10/2024

Step 1

It seems like we are given the density of bentene and volumes of some unknown substances. However, the problem does not provide enough information about what we are supposed to do with these volumes or how they relate to the reaction given. The reaction given is Show more…

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Transcript

00:02 Hey there, in this question we are trying to produce 1 .5 times 10, i believe it's to the third.

00:11 I'm having a little trouble reading that exponent, but if i use the third, the answer will work out to one of the options there.

00:19 So we're trying to produce this much energy from the reaction that is given to us.

00:24 Well, from that reaction, we see that for every two moles of the benzene, we can produce negative 6 ,278 kilojoules of energy.

00:39 All right.

00:41 So using that negative 6 ,278 kilojoules in every for every two moles of benzene that react.

01:00 All right, so i'm using that as a conversion factor here, and i don't really need the negative sign.

01:08 We know that's being given off, and that's also what we're trying to solve for is the amount given off, so we could put in our two negatives or just eliminate them because they're going to cancel.

01:19 All right, so this allows the kilojoules to cancel, and we now have moles of benzene.

01:27 Well, our next step then is going to be to convert moles to grams so that we can use our density to determine the volume in milliliters.

01:36 So we need the molar mass to convert from moles to grams because molar mass gives us the mass of one mole of any substance in grams.

01:46 And to determine that molar mass, we need to add together the masses for the elements in the compound.

01:52 Out.

01:53 So six times the mass of carbon plus six times the mass of hydrogen gives us 78 .12 grams of benzene in every mole...

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