please help

1. Define each of the following terms. You need not use complete sentences, but l expect reasonable spelling and grammar. a) Energy b) Heat c) Temperature d) Specific heat capacity 2. You hold a ball 6 feet above the ground. You release it and it falls due to the influence of gravity. a) Is it gaining or losing potential energy? b) Is it becoming more stable or less stable energetically? c) Is the process of falling endothermic or exothermic? 3. Everything is made up of particies - atoms and molecules. What happens to those particles as the substance is heated? Are the particles gaining just potential energy, gaining just kinetic energy, or both forms of energy? Explain. 4. You've been heating a beaker of water on a ring stand as part of an experiment. In cleaning up after your experiment, you start to unfasten the iron ring before it has a chance to cool fully, the iron ring feels hot. a) Is heat flowing from your hand to the iron ring. or from the iron ring to your hand? b). Is the process endothermic or exothermic for your hand? c) According to the concept of Conservation of Energy, how does the quantity of heat lost by the ring compare with. the quantity of heat gained by your hand? 5. What does it mean to say that a substance has a high specific heat capacity? In other words, if it has a high specific heat, does the substance conduct heat efficiently or not very well? 6. Iron has a specific heat capacity of 0.45J/gC; the specific heat capacity of aluminum is 0.90J/gC. What does that tell you about iron and aluminum in terms of how quickly they heat up and cool down? 7. Suppose you have rods of iron and aluminum, both the same size and shape, and painted to make them look alike. If you held the iron rod in one hand, and the aluminum rod in the other, and dipped them both in boiling water, how would you be able to tell which is which? 8. What quantity of heat is required to raise the temperature of 22 grams of aluminum from 25C to 55 C? Calculations must be shown. (See question 6 for values of C.) 9. What quantity of heat is required to raise the temperature of 22 grams of iron from 25 to 559C ? Calculations must be shown. (See question 6.) 10. If 1.0102J of heat is transferred to 1.0102g of iron initially at 15C, what will be the final temperature of the iron? Name 11. A 75-g piece of an unknown solid is heated to 98.2C. It is then dropped into 100 . Grams of water, initially at 15.0C. The final temperature of the system is 21.4C. The specific heat capacity of water is 4.18J/gC. Answer the following questions about this system. Show your calculations. a) What quantity of heat flows into the water? b) What quantity of heat must have been released by the unknown solid? c) What is the specific heat capacity of the unknown solid? 12. Suppose you add 25mL of water at 40.C to 25mL of water at 20.9C. a) Ideally, what would be the expected value of the final temperature after mixing? b) In a real-world situation, would you expect the final temperature be greater than 30 ? C, less than 30 . C, or exactly 30,C. Explain why you chose the option you picked