-Calorimetry Questions 1. A 24.6 g sample of nickel is heated to 110.0 °C and then placed in a coffee-cup calorimeter containing 125 g of water at a temperature of 23.00 °C. After the nickel cools, the final temperature of the metal and water is 24.83 °C. Assuming that no heat has escaped to the surroundings or has been absorbed by the calorimeter, calculate the specific heat of nickel. 2. When solutions of an acid and a base are mixed, heat is released. Using a coffee-cup calorimeter, 100.0 mL of 0.100 mol/L HCI are mixed with 100.0 mL 0.100 mol/L NaOH solution. The initial temperature of the solutions were 22.6 °C, and the temperature after mixing was 32.4 °C. Calculate the molar enthalpy of neutralization for the reaction: HCI (aq) + NaOH (aq) → NaCI (aq) + H,0 (1)

-Calorimetry Questions 1. A 24.6 g sample of nickel is heated to 110.0 °C and then placed in a coffee-cup calorimeter containing 125 g of water at a temperature of 23.00 °C. After the nickel cools, the final temperature of the metal and water is 24.83 °C. Assuming that no heat has escaped to the surroundings or has been absorbed by the calorimeter, calculate the specific heat of nickel. 2. When solutions of an acid and a base are mixed, heat is released. Using a coffee-cup calorimeter, 100.0 mL of 0.100 mol/L HCI are mixed with 100.0 mL 0.100 mol/L NaOH solution. The initial temperature of the solutions were 22.6 °C, and the temperature after mixing was 32.4 °C. Calculate the molar enthalpy of neutralization for the reaction: HCI (aq) + NaOH (aq) → NaCI (aq) + H,0 (1)

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

A 234.66 gram aqueous solution has a specific heat of 4.186 J/gºC. The solution is at 28.1 °C. What is the temperature of the solution in °C after 54.93 kJ of heat has been added to it?
6. Calculate the amount of heat released when 1.26 x 104 grams of ammonia NH3 are produced according to the following equation. N₂ + 3H₂ → 2NH3 AH = -92.6 kJ
A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants Periodic Table Part A q = specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the sblution increases to 30.0 °C At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, qp; that is, Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water (4.18 J/(g. °C)J, that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the suroundings. ΔΗp Express the…
3
30 g of HCL is mixed with 200 g of water. The water temperature changes from 24.6 to 28.2 °C. What was the heat change (enthalpy change) of the water?
Please help me complete this question
1 A piece of metal with a specific heat of 1.011 J/gºC is heated to 123.1ºC and then placed in 111.031 g of water which is at a temperature of 3.6 ºC. After a minute, the temperature of the water has stopped changing and is now 55.8ºC. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/gºC. Enter your answer with at least 3 sig figs.
Which of the reactions are exothermic? 2 Mg(s) + O,(g) → 2 MgO(s) + heat O NH, (g) + HCI(g) → NH,CI(s) + heat AgCl(s) + heat – Ag*(aq) + Cl¯(aq) 2 Fe, 0, (s) + 3 C(s) + heat → 4Fe(s) + 3 CO, (g) O C(graphite) + 0,(g) → CO,(g) + heat O CH, (g) + 20,(g) → CO,(g) + 2 H,O(1) + heat
2 moles of lithium metal reacts with liquid water to produce solid lithium hydroxide, hydrogen gas, and 402.4 kJ/mol of heat energy. a) write a balanced thermochemical equation for the reaction b) how much heat would be produced by the reaction of 14 g of lithium with an excess of liquid water c) is the reaction endothermic or exothermic?
A 4.81 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. If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt? How many moles of the unknown salt were used in the reaction ? _______ J?
1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.