The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1J/s). The plants in an agricultural field produce the equivalent of 23 kg of sucrose (C12H22 O11) per hour per hectare (1 ha = 10,000 m²). Assuming that sucrose is produced by the reaction 12CO2 (g) +11H₂O(l) → C12H22 O11 (s) + 1202 (9) 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= %

The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1J/s). The plants in an agricultural field produce the equivalent of 23 kg of sucrose (C12H22 O11) per hour per hectare (1 ha = 10,000 m²). Assuming that sucrose is produced by the reaction 12CO2 (g) +11H₂O(l) → C12H22 O11 (s) + 1202 (9) 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= %

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The energy associated with chemical processes is often quoted in kilojoules per mole of reactants. Please derive the conversion factor from eV/molecule to kJ/mol. (1 eV = 60218 × 10-19 J, 1 mole = 6.02214076 × 1023).
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 3.50 kg of water at 38.6 °C. During the reaction 131. kJ of heat flows out of the flask and into the bath.Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g^−1K^−1. Round your answer to 3 significant digits.
A large sport utility vehicle has a mass of 2500 kg.Calculate the mass of CO2 emitted into the atmosphere upon accelerating the SUV from 0.0 mph to 65.0 mph. Assume that the required energy comes from the combustion of octane (C8H18) with 30% efficiency. (Hint: Use KE = ½ mv2 to calculate the kinetic energy required for the acceleration and pay attention to units).
The copper mineral chalcocite, Cu2S, can be converted to copper simply by heating in air: Cu,S(s) + 0,(g) → 2Cu(s) + SO, (g)
(a) What is the theoretical yield of ammonia (in grams) if 16.55 grams of nitrogen gas and 10.15 grams of hydrogen gas are allowed to react? (b)Based on your theoretical yield, what is the percent yield of ammonia if only 8.33 grams of ammonia are produced? (c)How much heat energy (in kJ) will be absorbed or released if 8.33 grams of ammonia are produced? State whether the energy will be absorbed or released.
We can use Hess's Law (and some creativity!) to learn about the energetics of reactions that occur in remote environments. Consider the atmospheric reaction, NO + O → NO2 (a) Use the dissociation energy of O2, 498.34 kJ/mol, and the standard heats of formation for NO (+90.25 kJ/mol) and NO2 (+33.18 kJ/mol) to derive the enthalpy change for this reaction.
What are the pros and cons of the utilization of hydrogen gas as a source of energy? What are the obstacles that have prevented its widespread use?
The combustion of methane is described by the equation in the figure. How much energy would be released when 2.00 mole of methane is combusted? * AH = -890 kJ / mol +202(g) 4(g) → COx, +2H,0)
The reaction of A to produce B by the reaction 2A + C → B is exothermic with a ΔH = -345 kJ. If 25.0 g of A (MW = 68.45 g/mol) are reacted, how many grams of ice (heat of fusion = 6.01 kJ/mol) could be melted with the released energy?
The enthalpy of combustion of isooctane (C8H18), one of the many hydrocarbons in gasoline is 5.45 × 103 kJ/mol. Calculate the enthalpy change per gram of isooctane and per liter of isooctane (d = 0.688 g/mL).
If the reaction below produces 5,230 kJ of energy, how many grams of KCl will be produced? (KCl = 74.6 g/mol) 2 K (s) + Cl2 (g) → 2 KCl (g) ΔHrxn = –873.0 kJ
A 500 MW power plant burns bituminous coal having a heatingvalue 28,400 kJ/kg. The overall plant efficiency is 36 percent. The plant operates at an annual capacity factor of 65 percent, meaning that the electrical energy generated in a year is 65 percent of the maximum possible. Calculate the annual quantity (mass) of coal burned at this power plant. Also calculate the annual quantities of ash and sulfur in the coal entering the plant.