25.0 grams of calcium chloride are allowed to dissolve in 100.0mL in an insulated styrofoam calorimeter. The temperature of the water before calcium chloride is added is 22.0 degrees celsius. After dissolving, the maximum temperature of the solution is 73.6 degrees celsius.
a) Calculate the heat absorbed by the water.
b) Is this q(p) or q(v)?
c) Calculate deltaH for the reaction CaCl2(s) yields CaCl2(aq) (units should be kJ per mole.)
d) Is deltaH any different from deltaE for this reaction? Explain.
25.0 grams of calcium chloride are allowed to dissolve in 100.0mL in an insulated styrofoam calorimeter....
A coffee cup calorimeter initially contains 135g of water at 22.0oC. Calcium chloride (21.0g) at the same temperature is added to the water and after the CaCl2 dissolves the final temperature 46.0 degrees C. Calculate the molar enthalpy change for dissolving the salt in KJ/mol. Assume the solution has a heat capacity of 4.184 J/C g and assume no heat is lost to the surrounding or the calorimeter.
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)
When 0.1002g o ammonium chloride is dissolved in 225mL of water in a constant pressure calorimeter, the temperature drops from 25.3 degrees celsius to 13.4 degrees celsius. What is the heat absorbed or released per gram and per mole of ammonium chloride.
4. In an experiment, when 23.6 of calcium chloride, CaCl2 were dissolved in water in a coffee- cup calorimeter (at constant pressure), the temperature rose from 25.0°C to 38.7°C. The dissolution process is: CaCiz(s) - Ca2+ (aq) + 2C1-(aq) The heat capacity of the solution and the calorimeter is 1258 J/°C. The molar mass of CaCl2 is 110.98 g/mol. 1) Determine the heat that was absorbed by the solution and calorimeter. (1 point) 2) Determine the heat that was released...
Consider the dissolution of Calcium Chloride: CaCl2(s)---->Ca^+2(aq) + 2Cl−(aq) ΔHrxn= -81.5kJ An 12.0 g sample of calcium chloride is dissolved in 100.0 g of water, with both substance at 22.0 degree C. Molar Mass: CaCl2= 110.98g.mol Molar Mass H20= 18.02g/mol Density of H20= 1.00g/mol Cs(soln)= 4.20 J/(g K) Will the temperature of the solution go up or down? Explain. Calculate q(reaction)
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...
Thermometer When a solid dissolves in water, heat may be evolved or absorbed. The heat of aissolution (dissolving) can be determined using a coffee cup calorimeter. Cardboard or Styrofoam lid In the laboratory a general chemistry student finds that when 11.13 g of CsBr(s) are dissolved in 114.50 g of water, the temperature of the solution drops from 25.61 to 22.35 °C The heat capacity of the calorimeter (sometimes refered to as the calorimeteγ constant) was determined in a separate...
help with all of them pleaseee Extra Credit 4. In an experiment, when 23.6 of calcium chloride, CaCl2 were dissolved in water in a coffee- cup calorimeter (at constant pressure), the temperature rose from 25.0°C to 38.7°C. The dissolution process is: CaCl (s) - Ca2+ (aq) + 2C1- (aq) The heat capacity of the solution and the calorimeter is 12581/°C. The molar mass of Calais 110.98 g/mol 1) Determine the heat that was absorbed by the solution and calorimeter. (1...
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solutiorn phase reaction. Thermometer Stirring rod A student heats 63.92 grams of iron to 98.03 °C and then drops it into a cup containing 75.92 grams of water at 24.47 °C. She measures the final temperature to be 30.66 °C The heat capacity of the calorimeter (sometimes referred to as the...
ReviewI Constants1 Periodic Table Part A A calorimeter is an insulated device in which a chemical reaction is contained By measuring the temperature change. ΔΤ, we can calculate the heat released or absorbed during the reaction using the following equation: A calorimeter contains 35.0 mL of water at 13.5 °C . when 1.20 g of X (a substance with a molar mass of 61.0 g/mol) is added, it dissolves via the reaction X+20)-X(ag) and the temperature of the solution increases...