The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase a similar product called "Heater Meals." Just pour water into the heater unit, wait a few minutes, and you have a hot meal. The source of energy in the heater is Mg(s) + 2 H₂O(l) → Mg(OH)2 (s) + H₂(g) Calculate the enthalpy change under standard conditions, in joules, for this reaction. What quantity of magnesium is needed to supply the energy required to warm 45 mL of water (d = 1.00 g/mL) from 20. °C to 95 °C? The specific heat capacity of water is 4.184 J/g °C. A, H* (kJ/mol) Compound Mg(OH)2 (s) H₂O(l) -924.54 -285.83 AFER MEALD The "heater meal" uses the reaction of magnesium with water as a source of energy as heat. Enthalpy change = J/mol-rxn g Mg

The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase a similar product called "Heater Meals." Just pour water into the heater unit, wait a few minutes, and you have a hot meal. The source of energy in the heater is Mg(s) + 2 H₂O(l) → Mg(OH)2 (s) + H₂(g) Calculate the enthalpy change under standard conditions, in joules, for this reaction. What quantity of magnesium is needed to supply the energy required to warm 45 mL of water (d = 1.00 g/mL) from 20. °C to 95 °C? The specific heat capacity of water is 4.184 J/g °C. A, H* (kJ/mol) Compound Mg(OH)2 (s) H₂O(l) -924.54 -285.83 AFER MEALD The "heater meal" uses the reaction of magnesium with water as a source of energy as heat. Enthalpy change = J/mol-rxn g Mg

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

Related questions

Q: A 1.45 g sample of acetic acid , HC2H3O2 was burned in excess oxygen in a bomb calorimeter. The…

A: We have to predict the heat of combustion.

Q: A scientist measures the standard enthalpy change for the following reaction to be 74.8 kJ: 2HBr(g)…

A: Enthalpy of formation is the enthalpy change during the formation of one mole of the compound from…

Q: A 3.10 g sample of methane, CH4, is combusted in a calorimeter. The calorimeter and water combined…

A: Given: Mass of methane = 3.10 g Heat capacity of calorimeter and water = 41.50 kJ/K Rise in…

Q: In this experiment you will place a sample of your FeCl2 in water in a constant pressure calorimeter…

A: Heat is a form of energy that is exchanged between various temperature environments or objects…

Q: 14. A 222.5 mg sample of sucrose (C12H22O11) is combusted in a bomb calorimeter. The temperature of…

Q: A 55.6 g sample of glass is put into a calorimeter (see sketch at right) that contains 300.0 g of…

Q: A 50.0 mL sample of a 1.00 M solution of MgSO4 is mixed with 50.0 mL of 2.00 M NaOH in a…

A: Given: Volume of MgSO4 = 50.0 mL Concentration of MgSO4 = 1.0 M Volume of NaOH = 50.0 mL…

Q: 1.435 g of naphthalene (C10H8) is burned in a bomb calorimeter. There is exactly 2000.0 g of water…

Q: C(s) + 2H,0(g) CO2(g) + 2H2(g) AH = ? 1) CO2(g) – C(s) + O2(g) AH = 393.5 KJ 2) 2H20(g) – 2H2(g) +…

Q: Suppose we combust a 0.794 g sample of hexane (C6H14, molar mass = 86.18 g/mol) in a bomb…

Q: You wish to find the enthalpy for the reaction 6 GeI₄ (s) + 14 NH₄I (s) → 3 Ge₂H₆ (l) + 7 N₂ (g) +…

A: The above question is based on the Hess's law: It is defined as the total change when happened…

Q: If 0.315 moles of hexane (C6H14) is combusted in a bomb calorimeter containing 5.65 liters of water,…

A: The reaction’s enthalpies are determined by the calorimeter. The reactions inside calorimeter are…

Q: A 1.922-g sample of methanol (CH3OH; molar mass 32.04 g/mol) is burned in a constant-volume bomb…

Q: In a coffee-cup calorimeter, 7.60 g of potassium bromide (KBr; MW 119 g/mol) is mixed with 150.0 g…

A: All the necessary calculations have been done in the following step.

Q: When a 4.26 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of…

A: Given : Mass of octane reacted = 4.26 g Change in temperature of calorimeter and water = 26.7 oC…

Q: Measurements show that the energy of a mixture of gaseous reactants decreases by 153. kJ during a…

A: According to the first law of thermodynamics, the total heat change of a system at constant pressure…

Q: A student performed the procedure described in the lab manual using 49.9 mL of 1.0 M HCI and 49.3 mL…

A: Molarity of HCl = 1.0 MVolume of HCl: 49.9 mLMolarity of NaOH = 1.0 MVolume of NaOH = 49.3 mLInitial…

Q: In parts 2, 3 and 4 of this lab, you will be conducting calorimetry experiments on neutralization…

A: In calorimeter, the heat of the reaction is calculated using the formula q=m×c×∆T where m is the…

Q: You wish to find the enthalpy for the reaction 6 GeI₄ (s) + 14 NH₄I (s) → 3 Ge₂H₆ (l) + 7 N₂ (g) +…

A: The objective of this question is to calculate the enthalpy change for the given reaction using the…

Q: Consider the reaction C12H22011 (s) + 12 O2 (g) → 12 CO2 (g) + 11 H20 (1) in which 11 g of sucrose,…

A: Given data: Mass of sucrose m =11g, Heat capacity C = 7.50 kJ/ o C Change in temperature dT = 21.6 o…

Q: A 56.8 g sample of polystyrene, which has a specific heat capacity of 1.880 J-g¹C¹, is put into a…

Q: Measurements show that the energy of a mixture of gaseous reactants decreases by 177. kJ during a…

Q: For the reaction N₂(g) + O2(g) → 2 NO(g), AH = 180.5 kJ How much energy is needed to generate 25…

A: Nitrogen reacts with oxygen to form nitrogen monoxide. The equation for the balanced chemical…

Q: An electrical heater adds 21.7 kJ of heat to a constant-volume calorimeter. The temperature of the…

A: When 21.7 kj of heat is added temperature rise is of 4.49°C.When 1.75 g methanol burnt temperature…

Q: A common technique for forming metal electrodes on electronic devices is evaporation in a vacuum. In…

A: Given Data: The enthalpy of vaporization (ΔHvap) for gold = 310.9 kJ/mol given mass of liquid gold…

Q: In a calorimeter, 300 mL of 0.22 mol/L of calcium chloride is mixed with 200 mL of 0.33 mol/L of…

A: Information of question

Q: A 53.1 g sample of aluminum is put into a calorimeter (see sketch at right) that contains 100.0 g of…

Q: A 50.0 mL sample of 0.5 M AgNO3(aq) is mixed with a 50.0 mL sample of 0.5 M NaI(aq) in a…

Q: Consider the reaction C12H22011 (s) + 12 O2 (g) → 12 CO2 (g) + 11 H20 (1) in which 10.3 g of…

Q: A quantity of 2.00 ×102 mL of 0.715 M HCl is mixed with 2.00 × 102 mL of 0.358 M Ba(OH)2 in a…

A: Molarity - ratio of number of moles of solute to the volume of solution in litres. Formula is,…

Q: 3. 50.0 mL of 1.0 M sodium hydroxide and 50.0 mL of 1.0 M hydrochloric acid, both at 22.5 °C, were…

A: Given :---- Mass of sodium hydroxide solution (mNaOH) = 50.0 gMass of hydrochloric acid solution…

Q: Measurements show that the energy of a mixture of gaseous reactants increases by 275. kJ during a…

A: Here we are given that, energy of a mixture of gaseous reactants increase by 275 kJ. Also 109 kJ of…

Q: Calcium hydroxide is prepared by adding calcium oxide to water: CaO (s) + H2O (l) → Ca(OH)2 (s)…

A: Given, Calcium hydroxide is prepared by adding calcium oxide to water: CaO (s) + H2O (l) → Ca(OH)2…

Q: oxygen. The calorimeter contained 4.86 kg of water. Calculate the heat exchanged with respect to the…

Q: A 1.37 g sample of butane, C4H10(g), was burned in a bomb calorimeter in the presence of excess…

A: Mass of butane = 1.37 g Initial temperature = 23.6°C Final temperature = 35.6°C Heat capacity of…

Q: A 55.1g sample of polystyrene, which has a specific heat capacity of 1.880·J·g−1°C−1, is put into a…

Q: A 1.800-g sample of phenol (C6H4O2) was burned in a bomb calorimeter whose total heat capacity is…

A: Total heat(q) produced by 1.800 g of phenol can be calculated using following expression…

Q: An electrical heater is used to add 19.75 kJ of heat to a constant-volume calorimeter. The…

Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase a similar product called "Heater Meals." Just pour water into the
heater unit, wait a few minutes, and you have a hot meal. The source of energy in the heater is
Mg(s) + 2 H₂O(l) → Mg(OH)2 (s) + H₂(g)
Calculate the enthalpy change under standard conditions, in joules, for this reaction. What quantity of magnesium is needed to supply the energy required to warm 45
mL of water (d = 1.00 g/mL) from 20. °C to 95 °C? The specific heat capacity of water is 4.184 J/g · °C.
Af HⓇ (kJ/mol)
Compound
Mg(OH)2 (s)
H₂O(l)
-924.54
-285.83
MEATER MEALS
The "heater meal" uses the reaction of magnesium with water as a source of energy as heat.
Enthalpy change =
J/mol-rxn
g Mg

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

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 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C. The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data. Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol). C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy
The combustion of titanium with oxygen produces titanium(IV) oxide: Ti(s)+O2(g)→TiO2(g) When 2.060 g of titanium is combusted in a calorimeter, the temperature of the calorimeter increases from 25.00°C to 91.60 °C. If the heat capacity of the calorimeter is 9.84 kJ/°C, what is the heat associated with the combustion of one mole of Ti in this calorimeter?
Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2H4O, by the following reaction.C2H4O(g) + H2O(l) ? HOCH2CH2OH(l)Use Hess's law to obtain the enthalpy change for this reaction from the following enthalpy changes.2 C2H4O(g) + 5 O2(g) ? 4 CO2(g) + 4 H2O(l) ?H = -2612.2 kJHOCH2CH2OH(l) + 5/2 O2(g) ? 2 CO2(g) + 3 H2O(l) ?H = -1189.8 kJ
A 2.30 g sample of ethanol, CH3CH2OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 4.89 K. If the heat capacity of the bomb is 663 J/K and it contains 2.57 kg of water, what is the enthalpy change per mole of ethanol combusted? The specific heat capacity of water is 4.18 J/g×K and the molar mass of ethanol is 46.07 g/mol.
When a 4.31 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.2 kJ/•C. The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane. Enter your answer numerically and in terms of kJ/mol.
Measurements show that the energy of a mixture of gaseous reactants decreases by 373. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 136. 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 3 x10 significant digits. exothermic Is the reaction exothermic or endothermic? endothermic
The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5 × 104 kJ of heat? 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ
A 56.5 g sample of iron is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The iron sample starts off at 86.7 °C and the temperature of the water starts off at 21.0 °C. When the temperature of the water stops changing it's 22.8 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to 2 significant digits. J 0₂-C x10 x thermometer insulated container water sample a calorimeter
A 56.1 g sample of polystyrene, which has a specific heat capacity of 1.880 J-g °C-1 is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 29.8 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits. °C thermometer. insulated container water sample. a calorimeter 區 OU Ar
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 0.3215 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.162×10 g of water. During the combustion the temperature increases from 25.15 to 27.48 °C. The heat capacity of water is 4.184 J glc-!. The heat capacity of the calorimeter was determined in a previous experiment to be 769.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O,(g) – → 5 H,O(1) + 14 CO2(g) + Energy Molar Heat of Combustion = kJ/mol
A 57.1 g sample of polystyrene, which has a specific heat capacity of 1.880 J-g¹C, is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 38.3 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the polystyrene sample. Be sure your answer is rounded to 3 significant digits. 0°C 0...º X
A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C