He placed the his temperature scale at o degree for the boiling point, and ent downward and placed the freezing point at 100 degrees 10. What did the physicist Amonton contribute to the understanding of hot and cold? Amonton was doing heating, and cooling experiments. He saw that when he cooled the object that when the temp dropped so did the pressure. So he thought what would happen if you kept pushing the pressure back.
Therefore, according to Hess’s law, the heat of reaction of the one reaction should be equal to the sum of the heats of reaction for the other two. This concept is sometimes referred to as the additivity of heats of reaction. The primary objective of this experiment is to confirm this law. The reactions we will use in this experiment are: 18 - 1 Computer 18 You will use a Styrofoam cup in a beaker as a calorimeter, as shown in Figure 1. For purposes of this experiment, you may assume that the heat loss to the calorimeter and the surrounding air is negligible.
(4 points) q = m × c × Δt Given: q=? m = 34.720g c = 4.18 j/(g x °C) Δt = 41.6°C - 25.2°C = 16.4°C q = (34.720g) (4.18 j/(g x °C) (16.4°C) q = 2380.13j You are trying to ﬁgure out the energy change of the water which is the surroundings in the lab. To do that you must take the mass of the metal, which for me was Aluminum, and multiply it by the heat capacity of the water, which was given, then multiply that by the change in temperature, which is the ﬁnal temperature of the mixture
What do you think would happen to the temperature of the ice if you added 6 tablespoons of salt instead of 2 tablespoons? 5. If there are charged particles that can move around in a substance, that substance is able to conduct electricity. So, do ionic compounds or covalent compounds conduct electricity when dissolved in water? Explain.
CuSO4 4. What is the molar mass for anhydrous (without water) copper(II) sulfate? 159.62 g/mol Result: Observation: Some gray white substances precipitated from the water in the crucible. Data: * Mass of purified crucible and lid 30.59g * Mass of crucible and lid and hydrate 31.57g * Mass of hydrate alone 31.57g- 30.59g = .98g * Mass of crucible and lid and dehydrate 31.11g * Mass of dehydrate alone .52g This lab shows that hydrates are made up of crystal solids and water,
In our lab we use a more sophisticated one which included a lid on the cup with an inserted thermometer and a stirrer. Thermochemistry is the study of the heat released or absorbed as a result of chemical reactions. The measurement of the total energy of a thermodynamic reaction is called enthalpy (q). This is the basis for Hess’s law which states that if two reactions are combined to yield a third reaction, the sum of the first two is equal to the third. The energy change is the same whether the process occurs in one step or many.
Andrea Gurke #8 Period 3 Chem Traditional Chem Unit 10- Thermodynamics- Book chapter 10 Objective Objective 1- Can define and distinguish between heat and temperature Temperature: measure of random motion (average kinetic energy) of components in a substance Heat: Flow of energy due to a temperature difference Temperature | Heat | How fast atoms are moving | Amount of energy | Measure of avg. kinetic energy | Flow of energy due to temperature difference | Measure of amount of energy | Form of energy | Speed limit | | Objective 2- Can define Specific heat capacity Specific Heat- Amount of energy it takes to change temperature of a substance by 1 degree Celsius Low Specific heat= LESS time to heat up/cool down= less energy High specific heat= MORE time to heat up/cool down= more energy Formula = Q= SxMx▲T Objective 3- Can perform simple calculations using the calorimetry equation (q=sm▲t) Q=1251 J Q= SxMx▲T S=X 1251 J= (x)(35.2)(25) M=35.2 g 1251/880=880x T1= 0 degree C 1.42 g/J T2=25 degree C Objective 4- Can perform complex calculations using the law of conservation of energy | metal | water | S (J/ degrees C) | ? | 4.184 | Mass | 75025 | 100 | Ti | 99.3 | 22.4 | Tf | 32.9 | 32.9 | Q= SxMx▲T Qmetal+Qwater=0 Q= -Q metal | water | SxMx▲T | -(SxMx▲T) | S(75.25 g) (32.9-99.3) | -(4.184)(100)(32.9-22.4) | S(-4996.3) | -(4393.2) | S= | .879 | Objective 5- Understand endothermic and exothermic processes, including their definitions and values of enthalpy Exothermic= process when energy (as heat) flows OUT OF THE SYSTEM Ex: ice freezing Endothermic= process when energy (as heat) flows INTO THE SYSTEM Ex: boiling of water
Fully simplify the expression, tanx1+ tan2x . Use the knowledge that sin x= -35 and π2≤x ≤ 3π2 to express your simplified expression as an exact answer in fraction form. 4 Heat loss from electric hot water systems is an environmental issue. It is recognised that the heat loss from a closed, full hot water tank is proportional to the surface area of the tank. Determine the ratio of the heat loss from a 1m3 cylindrical tank of optimum dimensions (that is, the dimensions of the cylindrical tank for which the heat loss is a minimum) to the heat loss from a cubic tank with the same volume.