CHE 320 8-2 Journal

A student wrote the following equation C6H12O6(s) + 602(g) → 6CO2(g) + 6H₂O(g) + energy Based on the fact that water vapour is a product, the logical conclusion is that the equation represents: Select one: Ophotosynthesis in an open system cellular respiration in a closed system combustion in a closed system combustion in an open system

What is the name of the process shown below and how does it work (be specific about what happens to the molecules involved)? Which class of biomolecules (protein, lipid, carbohydrate, nucleic acid) are involved in this particular reaction example? List at least 2 types of functions this class of macromolecules might be involved in biologically. CH₂OH CH₂OH CH2OH CH₂OH НО ОН он ОН н ОН OH ОН Н + H2O → HO ОН ОН н OH + НО ОН ОН Н ОН

During the combustion of 5.00 g of ethanol (C2H5OH) 35.5 kcal of energy are released. How many grams of ethanol must be burned to release 450. kcal of energy? Report your answer to 3 sig figs. Do not include units and do not put your answer in scientific notation.(hint: there are several ways to correctly do this problem. Dimensional analysis is one of them. But in this case there's an easier way, if you can think of it. Remember, enthalpy is extensive. That's the point of this question.)

A sample of 20.1 g of a candy bar was burned in a calorimeter. The calorimeter was calibrated to have a heat capacity of 8.72 kcal/°C. The heat released caused the temperature of the calorinmeter to increase 13.3°C. Calculate the food caloric content of the candy bar in nutritional calories per gram to three significant figures. Recall that 1 nutritional calorie (Cal) = 1 kcal.

+) b) H30 H2O

Write a balanced chemical equation based on the following description: butanoic acid, C,H,COOH(I) burns in air | What type of reaction is represented by the following equation: 2Na(s) + Cl2(g) → 2NACI(s) A) combination B) decomposition C) double displacement D) single displacement

A sample of 1.91 g of potato chips was burned in a calorimeter. The calorimeter was calibrated to have a heat capacity of 6.94 kcal/ °C. The heat released caused the temperature of the calorimeter to increase 1.36 °C. Calculate the food caloric content of the potato chips in nutritional calories per gram to three significant figures. Recall that 1 nutritional calorie (Cal) = 1 kcal.

A number of companies currently lease solar panels to homeowners to offset the home’s energy use. The total energy production of a certain residential solar system in suburban Maryland was 7581.62 kWh over the last calendar year. What mass of carbon dioxide did this solar system keep out of the atmosphere during that time, assuming that the energy consumed by this home Chapter 5 Worksheet "Chapter 5 Worksheet" by Montgomery College is licensed under CC BY 4.0 would otherwise have been supplied solely by coal-burning power plants (note that this isn’t a great assumption, as Maryland also has a nuclear power plant, solar and wind farms, and Montgomery County incinerates waste to generate electricity)? Keep in mind that power plants are inefficient, and are able to convert on average 33% of the heat generated by the combustion of coal into electricity. Assume that coal can be approximated as C(s) (again, not a great assumption, but sufficient for this problem). Use the following data to…

4-hydroxycoumarin (s) and ammonium acetate (s) react to form 4-aminocoumarin (s) and water (l). What is the reaction enthalpy? Standard enthalpy of formation: 4-hydroxycoumarin = -351 kj/mol Ammonium acetate = -615 kj/mol Water = 285 kj/mol 4-aminocoumarin = 405 kj/mol

Name these organic compounds: Η Η Η Η Η Η ||| C=C=C-H ||| Η Η Η Η Η II H — C =C=C=C=C - H ||||| Η structure Η Η Η Η Η Η H H Η Η Η | Η ||| H – C – C =C=C=C=C=CH ||||||| Η Η Η Η Η Η Η name Π Π Π

6H2O (l) + 6CO2 (g) → C6H12O6 (s) + 6O2 (g) ΔH = +2803 kJ/mol Calculate the amount of sunlight energy required (in kJ) by a plant to synthesize 75.0 g of glucose (C6H12O6).

From the discussion question from Module 5, recall the chemical equation for the combustion of gasoline (iso-octane, C8H18) is: 2C8H18  +  25O2  --->  16CO2 + 18H2O This means that 2 moles of iso-octane combine with 25 moles of CO2 to produce 16 moles of CO2 and 18 moles of water. This is important for understanding the impact of fossil fuel use on the atmosphere because burning one mole of fuel adds a lot of CO2. Thinking about this in terms of the stoichiometry, and change in concentration, suppose we had 1.0 mole of iso-octane dissolved in 1.0 m3 of atmosphere. That means the concentration of carbon-containing molecules would be 1 mole per cubic meter. However, ff we burned all that iso-octane and convert the C8H18 into CO2 the concentration of carbon-containing molecules increases.  How much does the concentration of carbon-containing molecules increase if 1.0 mole of C8H18 in 1.0 m3 of air is converted into CO2 as shown in the chemical equation above?

The heating of CuSO4. 5H2O(S) yields several transitions as a function of temperature. The table below gives the percentage of original mass lost as a function of the approximate temperature. Use these percentages to determine the sequence of decompositions and write chemical equations for each transition. percentage of original mass lost 14.5 29.0 36.0 51.5 67.0 70.5 approximate temperature (Degree C) 100 130 220 800 910 1020

The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1 J/s). The plants in an agricultural field produce the equivalent of 21 kg of sucrose (C12 H22 O11) per hour per hectare (1 ha = 10,000 m Assuming that sucrose is produced by the reaction m²). 12CO2 (9) + 11H2O(1) → C12H22O11(s) + 120O2(g) AH=5640 kJ calculate the percentage of sunlight used to produce the sucrose – that is, determine the efficiency of photosynthesis in this field. Percent efficiency

NUMBER 63 and 64 and 65

Ethylene (C2H4) plays an important role in the ripening of certain fruits and vegetables. It is sometimes supplemented under controlled conditions at produce—processing facilities but is also produced naturally by many fruit-bearing plants.  Although the actual process by which plants produce ethylene is a complex one, imagine that it is produced by the simple breakdown of glucose according to the equation: C6H12O6 (s)  --> 3 C2H4 (g) + 3 O2 (g)   Given S°= 212.1 J/molK, ▲G°= -910.56 kJ/mol and ▲H°= -1274.5 kJ/mol for C6H12O6 (s).   a.) Determine the sign of ▲S° for the reaction. b.) Calculate ▲S° for the reaction. c.) Using the tabulated ▲G° values in the appendix, calculate ▲G° for the reaction. d.) Above what temperature (in °C) is the reaction spontaneous? Hint: you will first have to calculate H° using tabulated values.

5. When meat is cooked, protein breaks down, as shown below. The degraded protein is able to undergo a Maillard reaction with glucose released from the breakdown of muscle glycogen. Using the structures below, explain how the proteins is "breaking down" and why this facilitates a Maillard reaction with the glucose. SH this peptide is part of a larger protein SH CH, CH2 NH но .CH heat or enzymes .CH NH2 and and water (H,0) H. CH2 CH2 H,C CH3 H2C CH3 : ČH3 ČH3 он OH