Which one of the following is not a state function ?
change in temperature |
||
internal energy |
||
enthalpy |
||
heat |
Calculate ΔH for the following reaction
C2H4 (g) + 6 F2 → 2 CF4 (g) + 4 HF (g)
from
H2 (g ) + F2 (g) → 2 HF (g) ΔH = - 537 kJ
C (s) + 2 F2 (g) → CF4 (g) ΔH = -680 kJ
2 C (g) + 2 H2 (g) → C2H4 (g) ΔH = + 52 kJ
-719 kJ |
||
- 815 kJ |
||
-1165 kJ |
||
-2486 kJ |
Calculate ΔHo for
C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l)
from
ΔHof C6H6 (l) = 49.0 kJ
ΔHof CO2 (g) = - 393.5 kJ
ΔHof H2O (l) = -285.8 k J
- 2361 kJ |
||
- 1208.7 kJ |
||
- 3169.4 kJ |
||
- 1454.6 kJ |
Which atom is the smallest ?
O |
||
B |
||
C |
||
Cl |
Which one of the following is not a state function ? change in temperature internal energy...
Calculate ΔHo for C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l) from ΔHof C6H6 (l) = 49.0 kJ ΔHof CO2 (g) = - 393.5 kJ ΔHof H2O (l) = -285.8 k J
Practice with Hess's Law and Standard Heats of Formation 1. (Example) The reaction C2H4 (g) + 6 F2 (g) → 2 CF4(g) + 4 HF (g) can be written as the sum of: C2H4 (9) ► 2 C(s) + 2 H2 (g) AH = -52.3 kJ/mol 2 C(s) + 4 F2 (9) ► 2 CF4(9) AH = -1360 kJ/mol 2 H2(g) + 2 F2 (g) → 4 HF (a) AH = -1074 kJ/mol C2H4(g) + 6 F2(g) → 2 CF4(g)...
Calculate the standard enthalpy of formation of gaseous carbon tetrafluoride (CF4) using the following thermochemical information: 2 HF(g) H2(g) + F2(g) H = +537 kJ 2 CF4(g) + 4 HF(g) C2H4(g) + 6 F2(g) H = +2486.3 kJ C2H4(g) 2 C(s) + 2 H2(g) H = -52.3 kJ Calculate the standard enthalpy of formation of gaseous carbon tetrafluoride (CF4) using the following thermochemical information: 2 HF(g) H2(g) + F2(g) H = +537 kJ 2 CF4(g) + 4 HF(g) C2H4(g) +...
What is the enthalpy of reaction, dH(rxn), for the following reaction? C2H4 (g). +. 6 F2 (g). --->. 2 CF4 (g). +.4 HF (g) dH(f) +52.3 -680 -268.5. kJ/mole dH(rxn) - +2486 kJ dH(rxn) = -2486 kJ o dH(rxn) = -2434 kJ • dH(rxn) = -1000.8 kJ
Calculate the standard enthalpy of formation of gaseous carbon tetrafluoride (CF4) using the following thermochemical information: Calculate the standard enthalpy of formation of gaseous carbon tetrafluoride (CF4) using the following thermochemical information: H2(g)F2(g) 2 HF(g) 2 CF4(g)4 HF(g) C2H4(g) +6 F2(g) C2H4(g)2 C(s) 2 H2(g) AH -537 kJ AH 2486.3 kJ AH -52.3 kJ ΔΗ - kJ
Calculate the standard enthalpy of formation of gaseous hydrogen fluoride (HF) using the following thermochemical information: C2H4(g) + 6 F2(g) 2 CF4(g) + 4 HF(g) H = -2486.3 kJ CF4(g) C(s) + 2 F2(g) H = +680 kJ C2H4(g) 2 C(s) + 2 H2(g) H = -52.3 kJ H = ??? kJ
Calculate the standard enthalpy of formation of gaseous hydrogen fluoride (HF) using the following thermochemical information: C2H4(g) + 6 F2(g) 2 CF4(g) + 4 HF(g) H = -2486.3 kJ CF4(g) C(s) + 2 F2(g) H = +680 kJ C2H4(g) 2 C(s) + 2 H2(g) H = -52.3 kJ H = ___?kJ The answer is not -589.3
Calculate the standard enthalpy of formation of gaseous hydrogen fluoride (HF) using the following thermochemical information: C2H4(g) + 6 F2(g) 2 CF4(g) + 4 HF(g) (delta)H = -2486.3 kJ CF4(g) C(s) + 2 F2(g) (delta)H = +680 kJ 2 C(s) + 2 H2(g) C2H4(g) (delta)H = +52.3 kJ (delta)H =__________ kJ
Use the following information to calculate the heat of formation of propane C3H8. 3 C (S-Graphite) + 4 H2 (g) —› C3H8 (g) 1. C (S-Graphite) + O2 (g) —› CO2 (g) ΔH = - 393.5 kJ 2. H2 (g) + ½ O2 (g) —› H2O (l) ΔH = - 285.8 kJ 3. C3H4 (g) + 4 O2 (g) —› 3 CO2 (g) + 2 H2O (l) ΔH = - 1937 kJ 4. C3H6 (g) + 9/2 O2 (g) —›...
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol