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It takes 463./kJmol to break an oxygen-hydrogen single bond. Calculate the maximum
Be sure your answer has the correct number of significant digits.
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- It takes 839./kJmol to break a carbon-carbon triple bond. Calculate the maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.It takes 163./kJmol to break an nitrogen-nitrogen single bond. Calculate the maximum wavelength of light for which an nitrogen-nitrogen single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.It takes 155./kJmol to break a fluorine-fluorine single bond. Calculate the maximum wavelength of light for which a fluorine-fluorine single bond could be broken by absorbing a single photon. Round your answer to 3 significant digits.
- It takes 157./kJmol to break a nitrogen-oxygen single bond. Calculate the maximum wavelength of light for which a nitrogen-oxygen single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.It takes 348./kJmol to break a carbon-carbon single bond. Calculate the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon. Round your answer to 3 significant digits.It takes 614./kJmol to break a carbon-carbon double bond. Calculate the maximum wavelength of light for which a carbon-carbon double bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits. convert to nm
- It takes 348. kJ/mol to break a carbon-carbon single bond. Calculate the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.It takes 498./kJmol to break an oxygen-oxygen double bond. Calculate the maximum wavelength of light for which an oxygen-oxygen double bond could be broken by absorbing a single photon. Round your answer to 3 significant digits.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.
- 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?Suppose that you have a solution containing a substance whose molecules have two quantum states corresponding to different orientations of a certain subgroup of atoms. The energy difference between these two molecular states is ΔE = 0.130 eV. You are running an experiment where no more than 5% percent of the molecules can be in the higher-energy state, or it will cause unacceptable noise. Can you run the experiment at room temperature, or do you need to cool your solution? Decide by determining the percentage of molecules in the higher-energy state. The percentage of molecules in the higher-energy state is_____ %.Consider the molecules: CH2=CH-CH=CH-CH=CH-CH=CH-CH=CH2. Let’s assume that the 10 electrons that make up the double bonds can exist everywhere along the carbon chains. The electrons can then be considered as particles in a box; the ends of the molecule correspond to the boundaries of the box with a finite or zero potential energy inside. In this “molecular box”, 2 electrons can occupy an energy level. What are quantum states that the electrons from this molecule can occupy in the ground state? What’s the smallest frequency of light that can excite the electron? Note that the length of a C-C bond is about 1.54A and the length of a C=C bond is 1.34A to allow you to estimate the length of the “molecular box”