[SANGAT MUDAH] Cara menghitung kalor reaksi pada kalorimeter (PART 2)
Summary
TLDRIn this educational video, the host discusses how to calculate the enthalpy of combustion using a calorimeter. The first problem involves the combustion of 8 grams of methane, resulting in a temperature rise from 25.5°C to 95°C in a 4-liter water calorimeter. Using the heat capacity of water and assuming the calorimeter's capacity is zero, the enthalpy of combustion is calculated to be -2184 kJ/mol. The second problem examines a reaction between nickel and CuSO4 solution, causing a 5°C temperature increase. The reaction's enthalpy is determined to be -4000 kJ/mol under standard conditions, showcasing the application of thermodynamics in chemical reactions.
Takeaways
- 🔍 The video discusses how to calculate the enthalpy change using a calorimeter.
- 🔥 The first problem involves the combustion of 8 grams of methane, resulting in a temperature rise in the calorimeter.
- 🌡️ The calorimeter's temperature increases from 25.5°C to 95°C due to the reaction.
- 💧 The calorimeter contains 4 liters of water, and the specific heat capacity of water is given as 4.2 J/g°C.
- ⚖️ The mass of the water in the calorimeter is calculated to be 4000 grams, assuming 1 liter is equivalent to 1 kilogram.
- 🔢 The change in temperature (ΔT) is calculated as the difference between the final and initial temperatures.
- 🔄 The enthalpy change of the reaction is calculated using the formula: \( \Delta H_{reaction} = -(mass_{water} \times c_{water} \times \Delta T) \).
- 🌐 The calorimeter's heat capacity is considered zero, simplifying the calculation.
- 🔄 The moles of methane burned are calculated by dividing the mass by the molar mass.
- 🔍 The final enthalpy change per mole of methane is determined by dividing the total enthalpy change by the moles of methane.
- 🧪 The second problem involves a reaction between nickel and a CuSO4 solution, causing a 5°C temperature increase in the solution.
Q & A
What is the mass of methane (CH4) burned in the first problem?
-The mass of methane (CH4) burned is 8 grams.
What is the initial and final temperature of the calorimeter in the first problem?
-The initial temperature is 25.5 degrees Celsius, and the final temperature is 95 degrees Celsius.
How much heat capacity does the calorimeter have in the first problem?
-The calorimeter is assumed to have a heat capacity of zero.
What is the heat capacity of water in the first problem?
-The heat capacity of water is 4.2 Joules per gram-degree Celsius.
How much heat is absorbed by the water in the first problem?
-The water absorbs 1092 kilojoules of heat.
What is the molar mass of methane (CH4) used in the first problem?
-The molar mass of methane (CH4) is 16 grams per mole.
What is the amount of methane (CH4) burned in moles in the first problem?
-Half a mole of methane (CH4) is burned.
What is the enthalpy change for the combustion of methane in kilojoules per mole in the first problem?
-The enthalpy change for the combustion of methane is -2184 kilojoules per mole.
What is the mass of nickel metal reacted with CuSO4 solution in the second problem?
-The mass of nickel metal reacted is 2.95 grams.
How much temperature increase is caused by the reaction of nickel metal with CuSO4 solution in the second problem?
-The reaction causes a 5-degree Celsius increase in the temperature of the solution.
What is the heat required to raise the temperature of the solution by 1 degree Celsius in the second problem?
-It requires 4 kilojoules of heat to raise the temperature of the solution by 1 degree Celsius.
What is the molar mass of nickel used in the second problem?
-The molar mass of nickel is 59 grams per mole.
How many moles of nickel are reacted in the second problem?
-0.05 moles of nickel are reacted.
What is the enthalpy change for the reaction of nickel with CuSO4 solution in kilojoules per mole in the second problem?
-The enthalpy change for the reaction is -40000 kilojoules per mole.
Outlines
Cette section est réservée aux utilisateurs payants. Améliorez votre compte pour accéder à cette section.
Améliorer maintenantMindmap
Cette section est réservée aux utilisateurs payants. Améliorez votre compte pour accéder à cette section.
Améliorer maintenantKeywords
Cette section est réservée aux utilisateurs payants. Améliorez votre compte pour accéder à cette section.
Améliorer maintenantHighlights
Cette section est réservée aux utilisateurs payants. Améliorez votre compte pour accéder à cette section.
Améliorer maintenantTranscripts
Cette section est réservée aux utilisateurs payants. Améliorez votre compte pour accéder à cette section.
Améliorer maintenantVoir Plus de Vidéos Connexes
5.0 / 5 (0 votes)