When 50.0 g of 0.200 M NaCl(aq) at 24.1 °C is added to 100.0 g of 0.100 M AgNO3(aq) at 24.1 °C in a calorimeter, the temperature increases to 25.2 °C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g °C, what is the amount of heat in J produced

A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 29.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g.°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? q = kJ What is the enthalpy of the reaction? AHrxn kJ/mol =

When the Cacl2(s) is added to water, the following reaction occurs. Cacl (s) – Ca²"(aq) + 2CI"(aq) AH = - 81.5 kJ A 24.1 g sample of Caclz is dissolved in water, with both substances at 25.0 °C. Calculate the final temperature (in °C) of the solution assuming no heat is lost to the surroundings, the final solution, containing Cacl2 and water, has a mass of 100.0 g and the solution has a specific heat capacity of 4.18 J °c-lg-1. The molar mass of CaCl2 = 110.98 g/mol Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to one (1) decimal place. Answer: 59.0 The correct answer is: 67.3

A 1.75 g sample of zinc metal is reacted with 128 g of 1.10 M hydrochloric acid solution in a constant-pressure calorimeter. The resulting solution changes in temperature from 22.58 °C to 22.97 °C. The hydrochloric acid is in excess. Based on this information, and estimating the solution's heat capacity as 4.18 Jg1 °C, what is the amount of heat, in joules, transferred in this reaction?

A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC.  After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 104.84 grams.  For this problem, assume the  specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures.  What is the heat transferred by this reaction, in Joules?

How many moles of butane, C4H10(l), must be burned to produce 234 kJ of heat under standard state conditions? (The heat of combustion for butane is −2855.7 kJ/mol.)

100.0 mL of 1.00 M HBr at 22.5 °C is combined with 100.0 mL of 1.00 M LiOH at 22.5 °C. The mixture reaches a temperature of 29.2 °C. Assume the density of the solutions is 1.00 g/mL and their specific heat capacity is the same as pure water. What is the molar heat of reaction?

When a 7.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 5.28 kJ⋅K^-1, the temperature decreases by 0.330 K Calculate the molar heat of solution of KSCN.

50.0mL of a solution of HCl is combined with 100.0mL of 1.15 M NaOH in a calorimeter. The reaction mixture is initially at 22.4 degrees C and the final temperature after reaction is 31.2 degrees C. What is the molarity of the HCl solution? ( Assume that there is an excess of base (so all of the HCl has reacted), that the specific heat of the reaction mixture is 0.96 cal/g degrees C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mol.)

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