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Ch.5 - Thermochemistry

Chapter 5, Problem 115

A 201-lb man decides to add to his exercise routine by walking up three flights of stairs (45 ft) 20 times per day. Hefigures that theworkrequired to increasehis potential energy in this way will permit him to eat an extra order of French fries, at 245 Cal, without adding to his weight. Is he correct in this assumption?

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Hi everyone here we have a question telling us that a 78.0 kg teen wants to lose the weight she gained from eating a piece of cake. That was 129 calories. She walks up and down a 15 m staircase 12 times a day to do so is this enough to lose the weight? So we're going to use the formula, potential energy equals mass, times acceleration of gravity, times distance. So our potential energy Will equal 78 0.0 kg, Times 9. meters per second squared times 15 m. And she's doing that 12 times a day, so times 12 And that equals 137,000 32.4 kilograms times meters squared times seconds amber squared. And that is equal to 137, point for jewels. And let's change that into kill jules. So we have our 137, 0.4 jewels and let's multiply that by one, kill a jewel Over 10 to the third jewels And that equals .73-4 kill jules and we need to know that one calorie Equals one kill calorie equals four point 184 kg jewels. So now we're going to take our 0.7 3-4 killed Jules, times one calorie Over 4. killer jewels. And our killer drills are going to cancel out here And that equals 32 .92 calories, 32 .92 calories is less than Our calories, so it is not enough. And that is our final answer. Thank you for watching. Bye.
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Textbook Question

We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction is the conversion of methane to ethane: 2 CH4(g) → C2H6(g) + H2(g) Calculate the ΔH° for this reaction using the following thermochemical data: CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ΔH° = -890.3 kJ 2 H2(g) + O2(g) → 2 H2O(l) H° = -571.6 kJ 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) ΔH° = -3120.8 kJ

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Textbook Question

From the following data for three prospective fuels, calculate which could provide the most energy per unit mass and per unit volume:

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Textbook Question
When magnesium metal is burned in air (Figure 3.6), two products are produced. One is magnesium oxide, MgO. The other is the product of the reaction of Mg with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas. (e) The standard enthalpy of formation of solid magnesium nitride is -461.08 kJ>mol. Calculate the standard enthalpy change for the reaction between magnesium metal and ammonia gas.
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Textbook Question

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Textbook Question

At 20 °C (approximately room temperature) the average velocity of N2 molecules in air is 1050 mph. (b) What is the kinetic energy (in J) of an N2 molecule moving at this speed?

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Textbook Question

Suppose an Olympic diver who weighs 52.0 kg executes a straight dive from a 10-m platform. At the apex of the dive, the diver is 10.8 m above the surface of the water. (a) What is the potential energy of the diver at the apex of the dive, relative to the surface of the water?

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