1 / 5

Converting Between Temperature and Energy for Solids and Liquids

Converting Between Temperature and Energy for Solids and Liquids. The relationship between temperature and kinetic energy is different for each substance. The relationship is expressed as specific heat for any substance. This is an empirical value.

mervin
Télécharger la présentation

Converting Between Temperature and Energy for Solids and Liquids

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Converting Between Temperature and Energy for Solids and Liquids The relationship between temperature and kinetic energy is different for each substance The relationship is expressed as specific heat for any substance. This is an empirical value. Specific Heat - J/g K

  2. Specific Heat of Water - 4.184 J/gK

  3. How much heat energy is needed to raise the temperature of 25 ml of water from 30 C to 40 C. Note: the specific heat of water is 4.18 J/g-K; assume the density of the water is 1.00 g ml -1. Mass of water = 25 grams  K = 10 K 25 g 4.18 J 10 K = 1120 J g K

  4. The temperature of a 600.0 ml sample of water decreases from 25.0 to 19.0 C. How much heat energy is being used up. Note: the specific heat of water is 4.18 J/g-K and the density of water is 1.00 g per ml. Mass water = 600 ml 1 gram = 600 g 1 ml  K = 25 - 19 = 6 K 600 g 4.18 J 6 K = 15000 J = 15 kJ g K

  5. A student mixes 50.0 ml of a 1 M HCl solution and 50.0 ml of a 1 M NaOH solution in a insulated calorimeter. The temperature of the resulting solution increases from 21.0 C to 27.5 C. Calculate enthalpy in kJ per mol HCl. The specific heat of water is 4.18 J/g-K. Assume the density of the solution is 1.0 g/ml. Enthalpy =  H = heat of reaction  K = 27.5 - 21 = 6.5  Hrxn= (100 g H2O) (4.18 J) (6.5 K) = 2717 J 1 kJ = -2.72 kJ g K 1000 J 50 ml 1 mol HCl = 0.05 mol HCl 1000 ml  Hmol = 1 mol -2.72 kJ = - 54.4 kJ/mol 0.05 mol

More Related