A certain microwave oven delivers 750 watts (J/s) of power to a coffee cup containing 35.1 g of water at 31.1°C. If the wavelength of microwaves in the oven is 9.75 cm, how long does it take, and how many photons must be absorbed, to make the water boil? The specific heat capacity of water is 4.18 J/°C'g and assume only the water absorbs the energy of the microwaves. photons

A certain microwave oven delivers 750 watts (J/s) of power to a coffee cup containing 35.1 g of water at 31.1°C. If the wavelength of microwaves in the oven is 9.75 cm, how long does it take, and how many photons must be absorbed, to make the water boil? The specific heat capacity of water is 4.18 J/°C'g and assume only the water absorbs the energy of the microwaves. photons

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 71QAP: Consider burning ethane gas, C2H6 in oxygen (combustion) forming CO2 and water. (a) How much energy...

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Of the five elements Sn, Si, Sb, O, Te, which has the most endothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? E(g)E+(g)+e
Consider burning ethane gas, C2H6 in oxygen (combustion) forming CO2 and water. (a) How much energy (in J) is produced in the combustion of one molecule of ethane? (b) What is the energy of a photon of ultraviolet light with a wavelength of 12.6 nm? (c) Compare your answers for (a) and (b).
Light in the infrared portion of the electromagnetic spectrum excites vibrations of certain molecules, causing them to move more rapidly. In this manner, infrared light can be used to heat a substance. If a 1000.-mW, 808-nm laser is used to heat a 50.0-mL sample of water from 22.0 o C to its boiling point, a) how many photons will the water absorb and b) what is the minimum amount of time this will take?
A container with 0.2450.245 L of water is placed in a microwave and radiated with electromagnetic energy with a wavelength of 14.114.1 cm. The temperature of the water rose by 72.172.1 °C. Calculate the number of photons that were absorbed by the water. Assume water has a density of 1.00 g·mL−11.00 g·mL−1 and a specific heat of 4.184 J·g−1·°C−14.184 J·g−1·°C−1.
Photoelectron spectroscopy applies the principle of the photoelectric effect to study orbital energies of atoms and mol ecules. High-energy radiation (usually UV or x-ray) is absorbed by a sample and an electron is ejected. The orbital energy can be calculated from the known energy of the radiation and the mea sured energy of the electron lost. The following energy differences were determined for several electron transitions: ∆E2→1 = 4.098x10-17 J ∆E3→£1 = 4.854x10-17 J ∆E5→1 = 5.242x10-17 J ∆E4→2 = 1.024x10-17 J Calculate ∆E and l of a photon emitted in the following transitions: (a) level 3 → 2; (b) level 4 → 1; (c) level 5→4.
Consider light with a wavelength of 5.41 × 10⁻¹⁰ m. How much heat is required to heat 1 cup (237 g) of water from 25 °C to 100 °C? (s(H₂O) = 4.184 J/g･°C)
Photoelectron spectroscopy applies the principle of the pho-toelectric effect to study orbital energies of atoms and mol-ecules. High-energy radiation (usually UV or x-ray) is absorbedby a sample and an electron is ejected. The orbital energy can becalculated from the known energy of the radiation and the mea-sured energy of the electron lost. The following energy differ-ences were determined for several electron transitions:ΔE 2→1=4.098X10⁻¹⁷J, ΔE 3→1=4.854X10⁻¹⁷J, ΔE 5→1=5.242X10⁻¹⁷J, ΔE 4→2=1.024X10⁻¹⁷J Calculate the energy change and the wavelength of a photon emitted in the following transitions:(a) Level 3→2 (b) Level4→1 (c) Level5→4
3. The blue color in fireworks is due to copper (1) chloride , (CuCI), is heated at a temperature of 1200 oC. What is the energy emitted at 4.50 x 102 nm by CuCI?
It takes 242. kJ/mol to break a chlorine-chlorine single bond. Calculate the maximum wavelength of light for which a chlorine-chlorine single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits. nm 0 10 X
Suppose that the microwave radiation has a wavelength of 12.4 cm. How many photons are required to heat 285 mL of coffee from 25.0 ∘C∘C to 62.0 ∘C∘C? Assume that the coffee has the same density, 0.997 g mL−1, and specific heat capacity, 4.184 J g−1 K−1, as water over this temperature range. Express the number of photons numerically.
The energy required to break one mole of hydrogen-hydrogen bonds in H2 is 436 kJ. What is the longest wavelength of light with sufficient energy to break a single hydrogen-hydrogen bond?
Photoelectron spectroscopy applies the principle of the photoelectric effect to study orbital energies of atoms and molecules. High-energy radiation (usually UV or x-ray) is absorbed by a sample and an electron is ejected. The orbital energy can be calculated from the known energy of the radiation and the measured energy of the electron lost. The following energy differences were determined for several electron transitions: ΔΕ2–1 : 4.098 × 10-¹7 J AE5-1 = 5.242 × 10-¹7 J ΔΕ3-1 - = 4.854 × 10-17 J AE4-2= 1.024 × 10-¹7 J Calculate AE and λ of a photon emitted in the following transitions: (a) level 3 → 2; (b) level 4 → 1; (c) level 5 → 4.

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