What is the standard enthalpy of formation for a compound? For a pure element in its standard state?
Step 1 of 3
Solution: Here, we are going to calculate and compare the energy of the photons emitted by the given two radio stations. Step1: According to Planck’s quantum theory of radiation, the amount of energy associated with a quantum(in case of light, the quantum of energy is often called photon) of radiation is proportional to the frequency of light, E = h ---(1), where h is a universal constant called Planck’s constant. is the frequency and E is the energy of a photon. Step2: Given, frequency of the photon = 1010 KHz = 1010 x 10 s 3 -1 [1 KHz = 1000 Hz = 1000 s ] -1 = 1.010 x 10 s 6 -1 -34 Planck's constant, h = 6.626 x 10 J.s Substituting the values in equation (1), we get, E = (6.626 x 10 J.s) x (1.010 x 10 s ) 6 -1 -28 = 6.69 x 10 J...
Textbook: Chemistry: A Molecular Approach
Author: Nivaldo J. Tro
The answer to “What is the standard enthalpy of formation for a compound? For a pure element in its standard state?” is broken down into a number of easy to follow steps, and 18 words. The full step-by-step solution to problem: 28E from chapter: 6 was answered by , our top Chemistry solution expert on 02/22/17, 04:35PM. This full solution covers the following key subjects: broadcasts, radio, Photons, Energy, partner. This expansive textbook survival guide covers 82 chapters, and 9464 solutions. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3. Since the solution to 28E from 6 chapter was answered, more than 284 students have viewed the full step-by-step answer. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247.