Thermochemistry. DO NOW The specific heat of ethanol is 2.44 J/g°C. How many kilojoules of energy...
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Transcript of Thermochemistry. DO NOW The specific heat of ethanol is 2.44 J/g°C. How many kilojoules of energy...
![Page 1: Thermochemistry. DO NOW The specific heat of ethanol is 2.44 J/g°C. How many kilojoules of energy are required to heat 50.0 g of ethanol from -20.0°C.](https://reader036.fdocuments.in/reader036/viewer/2022062301/56649ef15503460f94c0310c/html5/thumbnails/1.jpg)
Thermochemistry
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DO NOW
• The specific heat of ethanol is 2.44 J/g°C. How many kilojoules of energy are required to heat 50.0 g of ethanol from -20.0°C to 68°C?
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Objective
–Describe how calorimeters are used to measure heat flow.
–Construct thermochemical equations.
–Solve for enthalpy changes in chemical reactions by using heats of reaction.
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Calorimetry
• Calorimetry - the measurement of the heat into or out of a system for chemical and physical processes.–Based on the fact that the heat released
= the heat absorbed• The device used to measure the absorption
or release of heat in chemical or physical processes is called a “Calorimeter”
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Enthalpy
• Heat absorbed or released by a reaction at constant pressure
H = qq = H = m x C x T
Note: We cannot calculate the actual value of enthalpy, only the change in enthalpy
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Thermochemical equation
• Includes the ΔH as either a product or a reactant
CaO(s) + H2O(l) Ca(OH)2(s) + 65.2 kJ
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Heat of Reaction
H = Hproducts – Hreactants
Type of Reaction Sign of H Exothermic Negative
(Hproducts < Hreactants)Endothermic Positive
(Hproducts > Hreactants)
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Exothermic Reaction 2CO(g) + O2(g) 2CO2(g) H = -566.8 kJ
Or
2CO(g) + O2(g) 2CO2(g) + 566.8 kJ
Negative sign means energy is released
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10
Ene
rgy
Reactants Products®
Change is down
ΔH is <0= Exothermic (heat is given off)
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2CO(g) + O2(g) → 2CO2(g) + 566.8 kJE
nerg
y
Reactants Products®
2CO + O2
2CO2
566.8kJ given off
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Endothermic Reaction
2CO2(g) 2CO(g) + O2(g) H = +566.8 kJ
Or
2CO2(g) + 566.8 kJ 2CO(g) + O2(g)
Positive sign means energy is absorbed
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13
Ene
rgy
Reactants Products®
Change is upΔH is > 0
= Endothermic (heat is absorbed)
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CaCO3 → CaO + CO2E
nerg
y
Reactants Products®
2CO2(g)
2CO(g) + O2(g)
566.8 kJ absorbed
2CO2(g) + 566.8 kJ → 2CO(g) + O2(g)
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Chemistry Happens in
MOLES• An equation that includes energy is called a
thermochemical equation• CH4 + 2O2 ® CO2 + 2H2O + 802.2 kJ
–1 mole of CH4 releases 802.2 kJ of energy.
–When you make 802.2 kJ you also make 2 moles of water
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• The magnitude of ΔH is directly proportional to the amount of reactants or products.
• 1A + 2 B ----> 1C ΔH = -100 kJ • 1/2 A + 1B ----> 1/2 C ΔH = -50
kJ
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CH4 + 2O2 ® CO2 + 2H2O; ΔH = -802.2 kJ
Rewrite chemical equation as a thermochemical equation.
Exothermic or endothermic reaction?
If 3 moles of O2 react with excess CH4 how much heat will be produced?
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1CH4(g) + 2 O2(g) ® CO2(g) + 2 H2O(l) + 802.2 kJ
• If 10. 3 grams of CH4 are burned completely, how much heat will be produced?
10. 3 g CH4
16.05 g CH4
1 mol CH4
1 mol CH4
802.2 kJ
= 514 kJ
ΔH = -514 kJ, which means the heat is released for the reaction of 10.3 grams CH4
Ratio from balanced equation
Start with known valueConvert to moles Convert moles to desired unit
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4 NO(g) + 6 H2O(l) 4 NH3(g) + 5 O2(g) ΔH = +1170 kJ
• Based upon the thermochemical equation given, calculate the heat associated with the decomposition of 1.15 g of NO.
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2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(l) ΔH = -3120 kJ
• Calculate the mass of ethane, C2H6, which must be burned to produce 100 kJ of heat.
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Heat of Reaction
CaO(s) + H2O(l) Ca(OH)2(s) ΔH = -65.2 kJEn
thal
py (H
) CaO + H2O
Ca(OH)2
ΔH = -65.2 kJ