Energy Change in Reactions - Page 2
Questions
- Two 20.0-g ice cubes at -11.0 °C are placed into 265 g of water at 25.0 C. Assuming no energy is transferred to or from the surroundings, how do you calculate the final temperature of the water after all the ice melts?
- What is a device that can change chemical energy into electrical energy?
- How do endothermic reactions absorb heat?
- How much energy is needed to heat 500 g of water at 50 degrees C to 70 degrees C?
- When gasoline burns, it reacts with oxygen in the air and forms carbon dioxide and water vapour. How does the potential energy of the gasoline and oxygen compare with the potential energy of the carbon dioxide and water vapour?
- The melting of ice at body temperature is an endothermic procesd thus eating ice counteracts exothermic metabolic reaction how much ice would you eat to counteract the heat produced by eating 28.3g of peanuts a)78g b) 1100grams?
- If the energy level of the products is higher than that of the reactants is the reaction endothermic or exothermic?
- What happens to particles when you add heat energy?
- What kind of energy can see and sometimes feel as heat?
- How would I convert kinetic energy for one particle in six dimensions (x, y, z, and their time derivatives) from Cartesian to spherical coordinates? Note: #dotq = (delq)/(delt)#, and this is from a 1962 Statistical Mechanics textbook by Norman Davidson.
- Is water freezing to ice endothermic or exothermic? Natural gas burning?
- What are chemical reactions that absorb energy?
- What is the study of the changes in the energy that accompanies chemical reactions and physical changes?
- Will lowering the temperature raise the energy level of the particles?
- How much heat is lost from a block of solid gold when 2000 g of this gold (Au) cools from 1064 degrees C to 25 degrees C? (Cp(Au) = 0.128 J/g*degC)
- Which reaction of those listed is MOST exothermic?
- Fill in the blanks? Word bank color endothermic energy enthalpy exothermic less mass more products reactants grams heat of reaction heat of solution moles negative neutral positive solvent temperature
- How much energy is released when a 40.0 g sample of liquid water completely freezes at 0 °C?
- How can we calculate #DeltaS# for an isothermal process?
- A 55.0-g aluminum block initially at 27.5 C absorbs 725 J of heat. What is the final temperature of the aluminum?