High School
SAT
ACT
University
MCAT
LSAT
DAT

Calorimetry

Related Topics

Wize High School Grade 12 Chemistry Textbook > Energy Changes

Calorimetry

6 Activities

Wize High School Grade 12 Chemistry Textbook > Energy Changes

First Law of Thermodynamics

3 Activities

From the following reaction:

2C6H12O6(s)+2O2(g)→12CO2(g)+4H2O(l)ΔHrxn=−1680kJ/mol⋅rxn2C_6H_{12}O_6(s)+2O_2(g)→12CO_2(g)+4H_2O(l)\qquad \qquad ΔH_{rxn}=-1680kJ/mol\cdot rxn

When an unknown quantity of sugar (C6H12O6) is burned, it was determined that the internal energy of the system decreased by 960 kJ and that 15.7 kJ of work was done on the system. How many grams of sugar were present at the beginning of this specific reaction?
More Calorimetry Questions:
Heat of Vaporization for Hexane
Hexane is heated from 0oC to 50oC and the equilibrium vapour pressure increases from 0.06 atm to 0.53 atm.
Calculate the ΔvapH for hexanes.
Thermochemistry: Melting ice
The standard enthalpy of fusion for water, ΔHfusiono=6.01 kJ/mol.\Delta H^o_{\textrm{fusion}}=6.01\ \textrm{kJ/mol}. Calculate the energy required (in KJ) to convert 26.0 g of ice at 0oC to liquid water at 20oC.
Calorimetry: Final temperature calculation
The ΔHsoln for the process when solid sodium hydroxide (NaOH) dissolves in water is 44 kJ/mol. When a 10.0 g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0oC to _______oC. Assume that the solution has the same specific heat as liquid water, i.e. 4.18 J/gK.
Calorimetry: Heat of combustion
When 2g of rocket fuel, N2H4 is burned inside of a bomb-calorimeter, the temperature of the water rises from 22oC to 29oC. If there is 0.9kg of water and the heat capacity for the bomb is 822J/oC, what is the heat of the combustion for one mole of N2H4 in the bomb calorimeter?
Thermochemistry: Enthalpy change
The enthalpy of vaporization for water, ΔHovaporization = 40.7 kJ/mol. Determine the enthalpy change (in kJ) when 54.0 mL of water is condensed from steam at 100oC.
Thermochemistry: Melting ice
The standard enthalpy of fusion for water, ΔHfusiono=6.01 kJ/mol.\Delta H^o_{\textrm{fusion}}=6.01\ \textrm{kJ/mol}. Calculate the energy required (in KJ) to convert 26.0 g of ice at 0oC to liquid water at 20oC.
Calorimetry: Heat of combustion
When 2g of rocket fuel, N2H4 is burned inside of a bomb-calorimeter, the temperature of the water rises from 22oC to 29oC. If there is 0.9kg of water and the heat capacity for the bomb is 822J/oC, what is the heat of the combustion for one mole of N2H4 in the bomb calorimeter?
Calorimetry: Heat of combustion
When 2g of rocket fuel, N2H4 is burned inside of a bomb-calorimeter, the temperature of the water rises from 22oC to 29oC. If there is 0.9kg of water and the heat capacity for the bomb is 822J/oC, what is the heat of the combustion for one mole of N2H4 in the bomb calorimeter?
Enthalpy of Formation
What is the enthalpy of the following reaction when 0.35 g of Mg2+ is produced? Use the following information:
ΔH°f[Mg(OH)2(s)] = −924.5 kJ
ΔH°f[NH4+(aq)] = −132.5 kJ
Thermodynamics: Internal energy and Enthalpy
2.3 moles of an ideal gas initially at -12oC and 16 atm underwent a complete expansion against a constant external pressure of 1atm and did 1.1kJ of work. Calculate Δ𝑈, Δ𝐻, 𝑎𝑛𝑑 𝑞 for this process.
Calorimetry: Final temperature calculation
The ΔHsoln for the process when solid sodium hydroxide (NaOH) dissolves in water is 44 kJ/mol. When a 10.0 g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0oC to _______oC. Assume that the solution has the same specific heat as liquid water, i.e. 4.18 J/gK.
Calorimetry: Heat of reaction
0.23 g of ethanol (C2H5OH) was burned in a bomb calorimeter (constant
volume
) leading to a temperature change from 22.50oC to 23.81oC. If the heat capacity of the calorimeter is 5.2 kJ/K, what would be the amount of heat generated by the combustion of exactly one mole of ethanol? ___________
Calorimetry: Temperature change
1. A 56.0 g block of iron heated to 90 °C is placed in a 4.8 kg water bath at 20 °C. What will be the final temperature of the iron? heat capacity of iron c = 0.450 J /gK, heat capacity of water is 4.185 J/gK
Calorimetry: Temperature change
How much heat energy is required to raise the temperature of 35.0 g of Al (c = 0.902 J/g K) from 18 °C to 65 °C? If this much energy were instead used to raise the temperature of 2.0 L of water, by how much would the temperature of the water change? Round to the nearest oC.
Calorimetry: Heat of reaction
4. A bomb calorimeter assembly has a heat capacity of 650 J/°C. The assembly is placed in a 3.0 L water bath and 2.5g of a fuel compound is burned in excess oxygen. If the temperature of the water bath increases by 4.8 °C, what is the value of qrxn?
What is the amount of heat released per gram of compound burned?
Calorimetry: Heat capacity
5. A fuel compound is burned in a bomb calorimeter, releasing 458 kJ of heat. The temperature of the calorimeter assembly and surrounding 2.5 L water bath increases from 23.5 °C to 28.6 °C. What is the heat capacity of the calorimeter assembly?
Calorimetry
When 1.00 kg of lead (specific heat =0.13 J g-1°C-1) at 125oC is added to a quantity of water at 18.0°C, the final temperature of the lead-water mixture is 32.0°C. What is the volume of water present?
Note: the density of H2O(l) is 1.00g mL-1 and the specific heat capacity is 4.18J g-1 oC-1
A 2.00 mole sample of a monoatomic ideal gas is initially at 1.00 L and 1.00 atm. Calculate the total q, w, ΔE{\small \Delta\text{E}}and ΔH{\small \Delta \text{H}}when the final conditions are 0.500 L and 5.00 atm along the pathway where the volume is compressed first.
[Do NOT include units in your answers]
Thermochemistry: Energy required to melt ice
You are lost on an expedition and you need some water to drink. There is ice around at an ambient temperature of -22oC. Using the thermodynamic information below, how much energy is required to take 1 kg of ice and warm it up to water at 12oC.
cp,s(ice)=2.01 JK−1mol−1ΔHfuso=6.01 kJmol−1cp,s(water)=4.18 JK−1mol−1ΔHfuso=44.00 kJmol−1\begin{array}{lr} c_{p,s}(ice) = 2.01\ J K^{-1} mol^{-1} & \Delta H^o_{fus} = 6.01\ kJ mol^{-1} \\ c_{p,s}(water) = 4.18\ J K^{-1} mol^{-1} & \Delta H^o_{fus} = 44.00\ kJ mol^{-1} \end{array}
Heat of Vaporization for Hexane
Hexane is heated from 0oC to 50oC and the equilibrium vapour pressure increases from 0.06 atm to 0.53 atm.
a) Calculate the ΔvapH for hexanes.
b) The human nose can detect hexane at a partial pressure of 0.005 atm. Estimate the temperature at which we can no longer smell hexane.
Copper, Silver, water ,Gold, hydrogensulfide and have specific heats of 0.385, 0.235, 4.18, 0.129, and 1.342 Jg-1oC-1 respectively. Which of the following would need smallest quantity of heat to change the temperature of 5400kg by 65oC
An alkane’s vapour pressure at 25.00 °C is 6.00 kPa. What is its vapour pressure at 80.00 °C if the enthalpy of vaporization is 43.0 kJ/mol? (Give your answer in kPa)
Sucrose, C12H22O11, can be metabolized for energy in the body according to the reaction: C12H22O11 (s) + 12 O2 (g) →\rightarrow 12 CO2 (g) + 11 H2O (l) ΔHo = -5.65x103 kJ
How many grams of sucrose must be burned to raise the temperature of 50.0 kg of water by 1.00oC? The specific heat capacity of water is 4.184 J g-1 K-1.
Calorimetry: Heat of reaction
The temperature of a 12.58 g sample of calcium carbonate (CaCO3(s)) increases from 23.6oC to 38.2oC. If the specific heat capacity of calcium carbonate is 0.82 J/g K. How many joules of heat are absorbed?
Calorimetry: Energy of vaporization of water
How much energy is required to bring 1.00 g of liquid water from 35 °C to 165 °C water vapour? The enthalpy of vaporization of water is +40.7 kJ/mol, the specific heat capacity of liquid water is 4.18 J / g °C, and the specific heat capacity of water vapour is 1.87 J/g °C.
From the following reaction:
2C6H12O6(s)+2O2(g)→12CO2(g)+4H2O(l)ΔHrxn=−1680kJ2C_6H_{12} O_{6(s)}+2O_{2(g)} \to 12CO_{2(g)}+4H_2O_{(l)} \hspace{20pt} \Delta H_{rxn}=-1680 kJ
When an unknown quantity of sugar (C6H12O6) is burned, it was determined that the internal energy of the system decreased by 960 kJ and that 15.7 kJ of work was done on the system. How many grams of sugar were present at the beginning of this specific reaction?
A chemical compound has a molecular weight of 89.05 g/mol. 1.400 grams of this compound underwent complete combustion under constant pressure conditions in a calorimeter with a heat capacity of 2.980 × 103 J/ °C. The temperature went up by 11.95 °C. Calculate the standard heat of combustion of the compound.
Calorimetry: Heat capacity of calorimeter
The combustion of 1.00 mol of glucose (C6H12O6) gives off 2.82x103 kJ of heat (i.e. ΔHcomb = 2.82x103 kJ mol-1). If 1.80 g glucose (molar mass is 180) is burned in a bomb calorimeter and the temperature of the calorimeter increases from 19.00oC to 23.50oC, what is the heat capacity of the calorimeter (kJ/oC)?
Calorimetry: Heat requirement
How much heat is required to convert a 15.5 g ice cube at -5.00oC to liquid water at 0oC? (The specific heat of ice is 2.09 J/g K, the specific heat of water is 4.18 J/g K, and the ΔHfus for water=334 J/g).
Thermochemistry: Melting ice
The standard enthalpy of fusion for water, ΔHfusiono=6.01 kJ/mol.\Delta H^o_{\textrm{fusion}}=6.01\ \textrm{kJ/mol}. Calculate the energy required (in KJ) to convert 26.0 g of ice at 0oC to liquid water at 20oC.
Enthalpy: Heat of vaporization
The enthalpy of vaporization for water, ΔHovaporization = 40.7 kJ/mol. Determine the enthalpy change (in kJ) when 54.0 mL of water is condensed from steam at 100oC.
Calorimetry: Using Heat Qualitatively
Consider the following four samples, all initially at room temperature:
The glass cubes are cooled to the same low temperature, and each is placed into one of the containers of room temperature gas.
(a) If Container A had a lower final temperature at thermal equilibrium than Container B, which gas has the lower specific heat capacity?
Thermochemistry: Calorimetry
Consider the following balanced chemical equation:
2CℓF3(g)+2O2(g)→Cℓ2O(g)+3F2O(g)∆rH°=???2 CℓF_3(g) + 2 O_2(g) → Cℓ_2O (g) + 3 F_2O (g) \qquad ∆_rH° = ???
Substance△fH° @ 25°C (kJ/mol)CℓF3(g)??Cℓ2O(g)80.3F2O(g)–21.7F2(g)0\def\arraystretch{1.5} \begin{array}{|c|c|} \hline \rm Substance & △_fH° \ @ \ 25°C \ (kJ/mol) \\ \hline CℓF_3 (g) & ?? \\ \hline Cℓ_2O (g) & 80.3 \\ \hline F_2O (g) & – 21.7 \\ \hline F_2 (g) & 0 \\ \hline \end{array}
Thermochemistry: Calorimetry
Ethene gas (C2H4) reacts with fluorine gas according to the following balanced equation:
C2H4(g)+6F2(g)→2CF4(g)+4HF(g)ΔrH°=−3012 kJ/mol⋅rxn @ 25°CC_2H_4 (g) + 6 F_2 (g) → 2 CF_4 (g) + 4 HF (g) \qquadΔ_rH° = −3012\ kJ/mol·rxn\ @ \ 25°C
Substance△fH° @ 25°C(kJ/mol)C2H4(g)??F2(g)0CF4(g)–933HF(g)–273.3\def\arraystretch{1.5} \begin{array}{|c|c|} \hline \rm{Substance} & △_fH° \ @ \ 25°C(kJ/mol) \\ \hline C_2H_4 (g) & ?? \\ \hline F_2 (g) & 0 \\ \hline CF_4 (g) & – 933 \\ \hline HF (g) & – 273.3 \\ \hline \end{array}
Calculate ΔHof of SO2(g) given the following: (answer in kJ)
S(s)+1.5O2(g)→SO3(g),ΔH=−395.8kJS_{(s)}+1.5O_{2(g)}\to SO_{3(g)}, \Delta H=-395.8kJ
2SO2(g)+O2(g)→2SO3(g),ΔH=−198.2kJ2SO_{2(g)}+O_{2(g)}\to 2SO_{3(g)}, \Delta H=-198.2kJ
The standard enthalpy of formation for the amino acid glycine C2H5NO2(s) is –528 kJ/mol at 25°C. Which reaction below has an enthalpy change equal to this value?
Calorimetry
Equal masses of copper and iron are both heated to a temperature of 100°C. Each piece of hot metal is then placed into its own beaker containing 1 L of water. If both beakers start with the same initial temperature, which beaker of water will have the higher final temperature?
Additional information: Cu (specific heat = 0.377 J/g°C); Fe (specific heat = 0.450 J/g°C)
Calorimetry
The temperature of a 12.58 g sample of calcium carbonate (CaCO3 (s)) increases from 23.6oC to 38.2oC. If the specific heat of calcium carbonate is 0.82 J/g K, how many joules of heat are absorbed?
Thermochemistry Calculations
The standard enthalpy of fusion for water, ΔHofusion = 6.01 kJ/mol. Calculate the energy required (in kJ) to convert 26.0 g of ice at 0oC to liquid water at 20oC.
Thermochemistry: Enthalpy change
The enthalpy of vaporization for water, ΔHovaporization = 40.7 kJ/mol. Determine the enthalpy change (in kJ) when 54.0 mL of water is condensed from steam at 100oC.
Bomb Calorimetry
A fuel compound was burned in oxygen in a bomb calorimeter with a combined heat capacity of 56.5 k] / K (Bomb assembly and water). The temperature of the surrounding water bath increased from 23.5 to 34.6 °C as a result. Calculate ΔEsys\Delta E_{sys}for this process? Consider any change in pressure due to gaseous products to be negligible.
More First Law of Thermodynamics Questions:
Practice: First Law of Thermodynamics
Practice: Work Calculation
0.08 mole of nitrogen undergoes the following process. What is the work done on the gas?
Practice: Internal Energy
Which of the following processes always results in a positive change in internal energy of a system?
Practice: First Law of Thermodynamics
Practice: Work
0.08 mole of nitrogen undergoes the following process. What is the work done on the gas?
Thermodynamics: Internal energy and Enthalpy
2.3 moles of an ideal gas initially at -12oC and 16 atm underwent a complete expansion against a constant external pressure of 1atm and did 1.1kJ of work. Calculate Δ𝑈, Δ𝐻, 𝑎𝑛𝑑 𝑞 for this process.
You have a family of four living in a home. The home has a one large
window with k=1.05 [WmK], A=1.2 [m2]k=1.05\ \left[\frac{W}{mK}\right],\ A=1.2\ \left[m^2\right]. The house is
made of wood k=0.2[WmK]k=0.2\left[\frac{W}{mK}\right]and an exposed area of A=15 [m2]A=15\ \left[m^2\right].Given an outside temperature of 5 °C5\ \degree C and an inside temperature of 24 °C24\ \degree C, find the smallest heater than can maintain the internal temperature.
Worked Example
Practice: Isothermal Expansion
4 moles of neon was confined to a 8L flask initially at room temperature underwent an isothermal expansion into a vacuum at 348K. Calculate ∆𝑈, ∆𝐻, 𝑎𝑛𝑑 𝑞 for this process.
Thermodynamics
In the following reaction, assuming that the gases behave ideally, calculate the work at 25C and 101.3kPa
Thermodynamics: Work calculation
Determine the work done when a gas is allowed to expand from 25.0 L to 50.0 L against a constant pressure of 13.6 atm.
Work equation:
∆V=Vf=Vi
If an exothermic process releases 555 J of heat to the surroundings when the volume of the system is kept constant, how would the amount of heat released change if the system were allowed to expand instead?
Thermodynamics
2. If an exothermic process releases 555 J of heat to the surroundings when the volume of the system is kept constant, how would the amount of heat released change if the system were allowed to expand instead?
Thermodynamics: Bond enthalpy
The enthalpy of combustion for ethanol (C2H5OH) is -1370.7 kJ/mol. Calculate q, w, ΔH and ΔU when 45g of ethanol are burned at 1atm and 298K.
A 2.00 mole sample of a monoatomic ideal gas is initially at 1.00 L and 1.00 atm. Calculate the total q, w, ΔE{\small \Delta\text{E}}and ΔH{\small \Delta \text{H}}when the final conditions are 0.500 L and 5.00 atm along the pathway where the volume is compressed first.
[Do NOT include units in your answers]
Which statement below is INCORRECT?
Which statement below is INCORRECT?
An alkane’s vapour pressure at 25.00 °C is 6.00 kPa. What is its vapour pressure at 80.00 °C if the enthalpy of vaporization is 43.0 kJ/mol? (Give your answer in kPa)
Thermodynamics: Work Done by a Piston
In an auto shop, a hydraulic piston expands to lift a car into the air so the mechanic can access the oil pan under the car. When the piston expands, which of the following is true? You may consider the piston the system.
Calorimetry
A fuel compound was burned in oxygen in a bomb calorimeter with a combined heat capacity of 56.5 kJ / K (Bomb assembly and water). The temperature of the surrounding water bath increased from 23.5 to 34.6 °C as a result. Calculate ΔEsys\Delta E_{sys}for this process? Consider any change in pressure due to gaseous products to be negligible.
Thermodynamics: Reaction of Mg with HCl
A 10.0 g piece of Mg(s) is deposited in a container with a vast excess of HCl(aq). A reaction takes place forming hydrogen gas and Magnesium Chloride. Write a balanced chemical reaction for the transformation and calculate the work done by the system as a consequence of the reaction, if Pex = 1.1 atm and T = 298.15 K. You may assume ideal behaviour.
Calorimetry: Energy of vaporization of water
How much energy is required to bring 1.00 g of liquid water from 35 °C to 165 °C water vapour? The enthalpy of vaporization of water is +40.7 kJ/mol, the specific heat capacity of liquid water is 4.18 J / g °C, and the specific heat capacity of water vapour is 1.87 J/g °C.
From the following reaction:
2C6H12O6(s)+2O2(g)→12CO2(g)+4H2O(l)ΔHrxn=−1680kJ2C_6H_{12} O_{6(s)}+2O_{2(g)} \to 12CO_{2(g)}+4H_2O_{(l)} \hspace{20pt} \Delta H_{rxn}=-1680 kJ
When an unknown quantity of sugar (C6H12O6) is burned, it was determined that the internal energy of the system decreased by 960 kJ and that 15.7 kJ of work was done on the system. How many grams of sugar were present at the beginning of this specific reaction?
How much work is performed in Joules when 3.00 mols of N2(g) expands against 1 atm of external pressure via heating from 298 K to 498 K at constant pressure of 1 atm?
A chemical compound has a molecular weight of 89.05 g/mol. 1.400 grams of this compound underwent complete combustion under constant pressure conditions in a calorimeter with a heat capacity of 2.980 × 103 J/ °C. The temperature went up by 11.95 °C. Calculate the standard heat of combustion of the compound.
Calorimetry: Heat capacity of calorimeter
The combustion of 1.00 mol of glucose (C6H12O6) gives off 2.82x103 kJ of heat (i.e. ΔHcomb = 2.82x103 kJ mol-1). If 1.80 g glucose (molar mass is 180) is burned in a bomb calorimeter and the temperature of the calorimeter increases from 19.00oC to 23.50oC, what is the heat capacity of the calorimeter (kJ/oC)?
Calorimetry: Heat requirement
How much heat is required to convert a 15.5 g ice cube at -5.00oC to liquid water at 0oC? (The specific heat of ice is 2.09 J/g K, the specific heat of water is 4.18 J/g K, and the ΔHfus for water=334 J/g).
A Piston containing an 1.3 moles of an Ideal Gas undergoes a compression from 32 L to 27 L against a constant external pressure of 178 kPa. During this transformation the temperature does not change. Calculate the heat flow, q, for this transformation.
First Law of Thermodynamics
0.08 mole of nitrogen undergoes the following process. What is the work done on the gas?
A freshly baked pie is placed near an open window to cool. Which of the following statements best describes this situation?
Thermodynamics: Internal Energy
Which of the following processes always results in a positive change in internal energy of a system?
Thermodynamics: Heat and Work
Consider the following balanced chemical equation for the combustion of propane, C3H8:
C3H8(g)+5O2(g)→4H2O(ℓ)+3CO2(g)q<0C_3H_8 (g) + 5 O_2 (g) → 4 H_2O (ℓ) + 3 CO_2 (g) \qquad q < 0
Use this information to answer the next two questions. Choose one if the options inside the brackets
The enthalpy of combustion for ethanol (C2H5OH) is -1370.7 kJ/mol. Calculate q, w, ΔH and ΔU when 45g of ethanol are burned at 1atm and 298K.
Thermodynamics
4 moles of neon was confined to a 8L flask initially at room temperature underwent an isothermal expansion into a vacuum at 348K. Calculate ∆𝑈, ∆𝐻, 𝑎𝑛𝑑 𝑞 for this process.
Isothermal Expansion of an ideal gas:
Free Expansion into a vacuum:
Worked Example
Four moles of an ideal gas originally at 323 oC and 7.3 atm underwent a complete expansion against a constant external pressure of 1 atm and did 8kJ of work. Calculate q, ΔE, ΔH.
Solve for the missing initial variable (Vi):
hint: rearrange PV=nRT to do this!
Thermodynamics
16 grams of dry ice (CO2(s)) was placed in a piston with an initial volume of 4L and allowed to sublimate and warm to room temperature. The system then underwent a reversible isothermal expansion to a final pressure of 1.0 atm. Calculate ΔU, q and w for this process. You can assume that CO2(g) behaves as an ideal gas.
R=0.08206Latm/Kmol
R=8.314J/Kmol
Thermodynamics
1.8 moles of an ideal gas initially at -5 oC and 1.7 atm underwent a complete expansion against a constant external pressure of 1atm and did 1.1kJ of work. Calculate ∆𝑈, ∆𝐻, 𝑎𝑛𝑑 𝑞 for this process.
Step 1: Extract all relevant information from the problem
Step 2: We have three of four variables for the initial state so we solve for the fourth (R=0.08206Latm/Kmol)
Thermodynamics: Internal Energy
The enthalpy of combustion for ethanol (C2H5OH) is -1370.7 kJ/mol. Calculate q, w and ΔU when 45.0g of ethanol are burned at 1atm and 298K.
Answers need to be in scientific notation, with proper significant figures. Give all values in kJ.
Thermodynamics: Pressure-Volume Work
Which of these reactions involve pressure-volume work being done on the system?
Bomb Calorimetry
A fuel compound was burned in oxygen in a bomb calorimeter with a combined heat capacity of 56.5 k] / K (Bomb assembly and water). The temperature of the surrounding water bath increased from 23.5 to 34.6 °C as a result. Calculate ΔEsys\Delta E_{sys}for this process? Consider any change in pressure due to gaseous products to be negligible.
Thermodynamics: Work Done During Acid Digestion of Magnesium
A 10.0 g piece of Mg(s) is deposited in a container with a vast excess of HCl(aq). A reaction takes place forming hydrogen gas and Magnesium Chloride.
a) Write a balanced chemical reaction for the transformation
b) Calculate the work done by the system as a consequence of the reaction, if Pex = 1.1 atm and T = 298.15 K. You may assume ideal behaviour.
Thermodynamics: Pressure-Volume Work
A system composed of 4.50 L of N2 in a cylinder expands against an external pressure of 300 kPa until its volume is 6.30 L.
What is the value of w for this process?
What would the value of w be if the external pressure was 0 kPa?
A steam turbine uses some form of energy to evaporate water, heat the vapour and move a cylinder. We can think of this a constant pressure process, where H2O(l)→H2O(g)H_2O(l) → H_2O(g).
Complete the following sentences about this process by choosing one description per line. Enter the answers separated by a comma in the box below.
This process is exothermic / endothermic.