Explain why Carbon Dioxide is a gas at room temperature while a diamond is a solid even though they both have covalent bonds.
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Explain why Carbon Dioxide is a gas at room temperature while a diamond is a solid...
2. If you have two beakers of liquid, one containing hexane and one containing water, you will notice that one has a smell and the other does not. Explain which one you can smell (using the wafting technique) and why you can smell that one liquid over the other. Discuss the interparticle forces. Use complete sentences. Do not use any abbreviations. 3. For the following pairs, predict which compound would have the higher melting point and explain why by discussing...
explain why elemental chlorine (Cl2) is a gas at room temperature and pressure while iodine (I2) is a solid despite the fact that both have similar lewis structures. explain based on the relative strength of their intermolecular forces of attraction
Consider a sample of carbon dioxide solid at room temperature and pressure. This substance will change from solid to a gas under these conditions. Which of the following is correct about this change of state? A) melting, exothermic B) melting, endothermic C) sublimation, exothermic D) sublimation, endothermic
Consider a given volume of carbon dioxide gas at room temperature (20.00C). (Molar Mass of Carbon dioxide is: 44.0 x 10-3 kg mol-1 J). (i). Calculate the root-mean-square Speed, Vrms, of a molecule of the gas? The answer must be given in scientific notation and specified to an appropriate number of scientific figures. (ii). At what temperature would the root-mean-square-speed be half of that at room temperature?
Explain why diamond and graphite have such different properties even though they are both composed of carbon.
explain why elemental chlorine (Cl2) is a gas at room tempeature and pressure while iodine (I2) is a solid despite the fact that both have similar lewis structures. explain based on the relative strength of their intermolecular forced of attraction.
Diamond and graphite are both made of carbon. Diamond is an electrical insulator, is the hardest material in the word and is often used as a cutting tool. In drastic contrast, graphite is an excellent electrical conductor, is easy to be cut and is often used as a lubricant at high-temperature mechanical environments. You have learnt the covalent bond, the van der Waals bond and the hexagonal carbon ring. Please explain why the properties of diamond and graphite are so...
1. Gas Laws 50.0g of dry ice (solid carbon dioxide) is placed in an evacuated 2.50L container The carbon dioxide fully sublimes and comes to room temperature, 22.5°C A. Determine the pressure in the container. Calculate the pressure in atmospheres, bar, and PSI. B. The volume of the container is expanded to 4.00L. Calculate the new pressure in atmospheres and bar. C. If the system from Part B has 12.50g of a diatomic elemental gas added the new total pressure...
Dielectric constants measured at room temperature under 1000 Hz are 5.5 for diamond and 10 for graphite. Both diamond and graphite are single elemental crystals of carbon, why do their dielectric constants differ so much?
Solid cobalt(III) oxide reacts with solid carbon to form solid cobalt and carbon dioxide gas Express your answer as a chemical equation. Identify all of the phases in your answer.