Diamon and graphite are two crystalline forms of
carbon. At 1 atm and 25°C, diamond changes to graphite so slowly
that the enthalpy change of the process must be obtained
indirectly. Determine delta H rxn for C(diamond) >
C(graphite)
with equations from the following list:
Diamon and graphite are two crystalline forms of carbon. At 1 atm and 25°C, diamond changes...
Enter your answer in the provided box. Diamond and graphite are two crystalline forms of carbon. At 1 atm and 25°C, diamond changes to graphite so slowly that the enthalpy change of the process must be obtained indirectly. Determine A Hrxn for C(diamond) — Сgraphite) with equations from the following list: (1) C(diamond) + O2(g) + CO2(g) (2) 2 CO2(g) → 2 CO(g) + O2(8) (3) C(graphite) + O2(g) → CO2(g) (4) 2 CO(g) → C(graphite) + CO2(g) AH=-395.4 kJ...
1 out of 10 attemp Enter your ans wer in the provided box Diamond and graphite are two crystalline forms of carbon. At 1 atm and 25°C, diamond changes to graphite so slowly that the enthalpy change of the process must be obtained indirectly. DetermineA for rxn (diamond)- → C (graphite) C with equations from the following list: (1) Cdia (2) 2CO2(g)→2CO(g ) + O2(g) (3) C(graphite) +02(g)→CO2(g) (4) 2C0(g)→C(graphite) + CO2(g) AH AH-566.0 kJ AH--393.5 kJ AH--172.5kJ =-395.4 kJ...
carbon. Determine the AHrxn for C (diamond) → C (graphite), using the following thermochemical equations: a) C (diamond) + 02 (9) → CO2 (9) AH = -395.4 kJ b) CO (9) + 12 02 (9) → CO2 (9) AH = -283.0 kJ c) C (graphite) + CO2 (9) ► 2 CO (9) AH = +172.5 kJ
5. Use the following data to determine the delta H for the conversion of diamond into graphite: C(diamind) (s) + O2(g) = CO2(g) delta H degrees = -395.4 kJ 2CO2(g) = 2 CO(g) + O2(g) delta H degrees = 566.0 kJ 2CO(g) = C(graphite) (s) + CO2 (g) delta H degrees = -172.5 kJ C(diamond) (s) = C(graphite) delta H degrees = ?
19. Calculate AH° for the conversion of graphite into diamond from the following thermochemical equations. C(s, graphite) + O2(g) — C(s, diamond) + O2(g) CO2(g) AH° = -393.5 kJ + CO2(g) AH' = -395.9 kJ e uso -395.9 kJ +393.5 kJ -789.4 kJ +2.4 kJ -2.4 kJ
4. You are given the following information. C (graphite) + O2(g) — CO2 (g) CO(g) + 02 (g) - CO2 (g) Determine the standard enthalpy change for the reaction: C (graphite) + / O2 (g) - CO (g) AH° = - 393.5 kJ AH° = - 283.0 kJ AHrxn = ?
e. -1135 Given the following reactions: CaCO3 (s)-> Cao (s) + CO2 (g) C (s, graphite) + O2 (g)-> Co2 (g) AH-393.5 kJ the enthalpy of the reaction CaCO3 (s) -> CaO (s) + C (s, graphite) + O2 (g) ΔH = 178.1 kJ is kJ Select one: 4 a. 7.01 x 10 b. 571.6 ) c. 215.4 d. -215.4 ie. -571.6 Check Given the data in the table below, AH for the reaction
please help 4. You are given the following information. C (graphite) + O2 (g) - CO2 (g) CO(g) + 02 (9) - CO2 (g) Determine the standard enthalpy change for the reaction: C (graphite) + 02 (g) - CO(g) AH = - 393.5 kJ AH° = -283.0 kJ AHrxn = ?
3. (25 pts) Buckminsterfullerene is a molecule with the formula C. (60 atoms of carbon held together by covalent bonds). It was manufactured in 1985 at Rice University. Given the following data: CO2(g) + C(s, graphite) + O2(8) AH,° = +393.5 kJ 60 CO2 (g) → Co (s) + 60 02(8) AH2° = +25937 kJ Write the balanced standard enthalpy equation for the formation of solid Coo law to determine the standard enthalpy (or heat) formation of solid Co. Buckminsterfullere
PROBLEM-SOLVING CLASS ACTIVITY 11 Use Hess's Law to calculate the enthalpy of formation of CH2OH: C(graphite) + 2 H2(g) + 1026) → CH2OH(1) Given the following data: CH2OH() • 02(9) + CO2(g) + 2H2O(1) AH°: -726.4 kJ/mol C(graphite). O2(g) → CO2(9) AH' = -393.5 kJ/mol H2(g) + 40269) → H2O(1) AH = -285.8 kJ/mol