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specific heat capacity 2. If 3.8 g of calcium chloride (CaCl2) is dissolved in 100.0 mL...
LAB 10 PRE LAB WORKSHEET Specific Heat Capacity (C) The energy transferred as heat that is required to raise the temperature of 1 gram of a substance by 1 kelvin. q= - m x Cp X AT q=heat lost or gained, m= mass of solution (grams) Cp = the Specific Heat Capacity of a compound (J/g x °C)) AT = Tfinal-Tinitial AHsolution = 9 moles of salt 1. If 1.25 g of ammonium nitrate (NH4NO3) is dissolved in 25.0 mL...
(#3) How much heat energy is released by dissolving 10.0 g of CaCl2 in 100.0 mL of water?. Use formula q=mcAT. The specific heat of water is 4.184J/g C, and the density os water is 1.00 g/mL. Open the Endothermic and Exothermic Reactions Lab Activity (Section 6.5, Figure 6.9) to complete this worksheet. 1. Measure the temperature change after dissolving a 5 g sample of each substance in 100 mL of water. Determine which solutes have an exothermic dissolving process,...
0.50 g of calcium chloride (CaCl2) was added to a test tube holding 5 mL of distilled water. A temperature probe was placed in the test tube to record any change in temperature during the reaction. The baseline temperature of the water before adding the CaCl2 was 23.6 degrees Celsius. After the CaCl2 was added to the water the temperature of the solution peaked at 25.7 degrees Celsius. 1) Draw an energy diagram of the process and label the Energy...
(#5) How much heat is absorbed by dissolving 10.0 g of NaNO3 in 100.0 mL of water? Open the Endothermic and Exothermic Reactions Lab Activity (Section 6.5, Figure 6.9) to complete this worksheet. 1. Measure the temperature change after dissolving a 5 g sample of each substance in 100 mL of water. Determine which solutes have an exothermic dissolving process, and which have an endothermic dissolving process. Naci NaOH NaNO3 CaCl2 KOH NH4NO3 Temperature change (°C) 1-0.79 13.30 -2.88 |...
When 23.6 g of calcium chloride, CaCl2, was dissolved in water in a constant-pressure calorimeter, the temperature rose from 25.0 C to 38.7 C. If the heat capacity of the solution and the calorimeter is 1258 J/C, what is the enthalpy change when 0.710 mol of calcium chloride dissolves in water? The solution process is CaCl2(s) --> Ca2+(aq) + 2Cl–(aq)
8. A student conducts an experiment to determine the enthalpy of solution for lithium chloride dissolved in water. The student combines 5.00 grams of lithium chloride with 100.0 ml of distilled water. The initial temperature of the water is 23.0 °C and the highest temperature after mixing reaches 33.0 °C. Assume a density of 1.00 g.ml and a specific heat of 4.18 J/gºC. a. Is the reaction endothermic or exothermic? Justify your answer. b. Calculate the temperature change of the...
If the temperature of 100.0 mL of water rises from 25.0°C to 32.0°C, how much heat was added? Assume the density of water is 1.00 g/mL and the specific heat capacity of the water is 4.184 J/g°C. Include units and use the correct number of significant figures. Define the terms "exothermic" and "endothermic". What is the sign of AH associated with these two terms? Exothermic: Endothermic
Prepare yourself for the laboratory: Question #2 1.26 g of LiCl(s) is dissolved in 25.0 mL of water that is initially 21.0°C a) Write the chemical equation for the dissolution of LiCl(s) b) Using the thermodynamic tables in Appendix II of Tro, calculate the molar enthalpy of dissolving LiCI(s) in water. Is this process endothermic or exothermic? Calculate the amount of heat absorbed/released when 1.26 g of Licl(s) dissolves. c) d) Calculate the final temperature of the solution. You can...
1. 5.00 g of urea, (NH2)2CO is dissolved in 250.0 mL of water(density = 1.00 g/mL) at 30.0oC in a coffee cup calorimeter. When this is done, 27.6 kJ of heat is absorbed. (5 points) a) Is the solution process exothermic or endothermic? c) What is qwater? d) What is the final temperature of the solution(specific heat constant of water is 4.18 J/g.OC)? Please show all the work!! thank you very much :)
16.41 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.7°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g・°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.