Suppose that 125 mL of 0.1125 M HCI is reacted with 155 mL of 0.1010 M NaOH in a coffee-cup calorimeter. HCI(aq) + NaOH → H20(1) + NaCl(aq) -56 KJ mol AH = If the initial temperature of the mixture is 22.1°C, calculate the final temperature of the mixture given the following information. Ssolution 4.1 °C Dsolution = 1.02 - mL O 25.5 °C O 24.3 °C O 22.8 °C O 19.8 °C

Suppose that 125 mL of 0.1125 M HCI is reacted with 155 mL of 0.1010 M NaOH in a coffee-cup calorimeter. HCI(aq) + NaOH → H20(1) + NaCl(aq) -56 KJ mol AH = If the initial temperature of the mixture is 22.1°C, calculate the final temperature of the mixture given the following information. Ssolution 4.1 °C Dsolution = 1.02 - mL O 25.5 °C O 24.3 °C O 22.8 °C O 19.8 °C

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

When 130. mL of 0.204 M NaCl(aq) and 130. mL of 0.204 M AgNO3(aq), both at 21.1°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.6°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 2.71x10³ J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g.°C, and 0.997 g/mL, respectively). Using this data, calculate AH in kJ/mol of AgNO3(aq) for the given reaction. 4.0✔✓ kJ/mol
Measurements show that the energy of a mixture of gaseous reactants decreases by 178. kJ during certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -163. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Round your answer to 2 significant digits. Is the reaction exothermic or endothermic? kJ exothermic endothermic x10 X
A 55.1g sample of polystyrene, which has a specific heat capacity of 1.880·J·g−1°C−1, is put into a calorimeter (see sketch at right) that contains 200.0g of water. The temperature of the water starts off at 25.0°C. When the temperature of the water stops changing it's 31.9°C. The pressure remains constant at 1atm . Calculate the initial temperature of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits.
A chemist carefully measures the amount of heat needed to raise the temperature of a 533.0 mg sample of CH,N from 53.8 °C to 68.3 °C. The experiment shows that 16.5 J of heat are needed. What can the chemist report for the molar heat capacity of CH,N? Round your answer to 3 significant digits. -1 - 1 J•mol • K x10
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.9101 g sample of phthalic acid (C8H6O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.224×103 g of water. During the combustion the temperature increases from 28.19 to 31.02 °C. The heat capacity of water is 4.184 J g-1°C-1.The heat capacity of the calorimeter was determined in a previous experiment to be 876.0 J/°C.Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phthalic acid based on these data.C8H6O4(s) + (15/2) O2(g) 3 H2O(l) + 8 CO2(g) + EnergyMolar Heat of Combustion = ______________ kJ/mol
When 130. mL of 0.198 M NaCl(aq) and 130. mL of 0.198 M AgNO3(aq), both at 21.8°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 24.2°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 2.60 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g·°C, and 0.997 g/mL, respectively). Using this data, calculate ΔH in kJ/mol of AgNO3(aq) for the given reaction. This is the complete question, nothing was left out. Thank you
The reaction of zinc with hydrochloric acid is represented by the reactionZn(s) + 2 HCl(aq) ↔ ZnCl 2(aq) + H 2(g) -- ΔH = -152.5 kJ How many grams of zinc reacted with an excess of HCl (100.0 mL) if the temperature of the calorimeter increased from 25.0Â°C to 35.85 Â°C? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*Â°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.
You mix 125 mL of 0.250 M CSOH with 50.0 mL of 0.625 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.70 °C before mixing to 24.59 °C after the reaction. CsOH(aq) + HF (aq) → CsF(aq) + H₂O(l) What is the enthalpy of reaction per mole of CSOH? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g. K. Enthalpy of reaction = kJ/mol
Constants Periodic Table Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HC1(aq)→ZnCl2 (aq) + H2 (g) When 0.112 g of Zn(s) is combined with enough HCl to make 515 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.1 C to 241 °C. Part A Find A H for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g. C as the specific heat capacity.) να ΑΣφ AH,xn - kJ/mol Submit Previous Answers Request Answer * Incorrect; Try Again; 25 attempts remaining Next > Provide Feedback P 8:36
The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol
You have 8.99 g sample of an unknown salt (MM = 116.82 g/mol). It is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What is the Mass inside calorimeter (g)? Change in Temp inside calorimeter (C)? How much Heat gained (J)? Total Heat? How many mols of the unknown salt? What is the change in empalthy?
A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. Wht is the change in teperature in celcios inside the calometer? was the dissolution process endothermic or exothermic? how much heat, in J, was hained b the solution? assume the specific heat of the solution is the same as water, 4.184 J/g. celcius