AP Chem Unit 6.6-6.8

C+ O₂ --> CO₂ + 60kJ

what is the ΔH for the reaction?

• +60

• -60

• there is no way to know

How do you calculate Enthalpy of a reaction?

• ΔH = ΔH_products - ΔH_reactants

• ΔT = q / mC

• ΔG = ΔH -TΔS

• E = mc²

Which symbol represents Enthalpy change?

• ΔH

• ΔT

• ΔG

• ΔS

Calculate ΔH_rxn for the reaction of sulfur dioxide with oxygen. 2SO_2(g) + O_2(g) → 2SO_3(g)

(ΔH⁰_f (SO2) = –296.8 kJ/mol; ΔH⁰_f (SO3) = –395.7 kJ/mol)

• –98.9 kJ

• –197.8 kJ

• 98.9 kJ

• 197.8 kJ

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

The standard enthalpy changes of formation of iron(II) oxide, FeO(s), and aluminium oxide, Al₂O₃(s), are –266 kJ mol^–1 and –1676 kJ mol^–1 respectively.

What is the enthalpy change under standard conditions for the following reaction?

3FeO_(s) + 2Al _(s)  → 3Fe_(s) + Al₂O_3(s)

• +878kJ

• –878kJ

• –1942kJ

• –2474kJ

Tags

NGSS.HS-PS1-4

Using the table of average bond energies below the image, the ΔH for the reaction in kJ is.....

• + 160 kJ
• -63 kJ
• - 160 kJ
• -217 kJ

Tags

NGSS.HS-PS1-4

Given the equation I_2(s) + 62.4 kJ → I_2(g), which of the following is true?

• ΔH = +62.4 kJ

• The reaction is exothermic.

• ΔH = -62.4 kJ

• The reaction releases heat

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

How much energy is transferred from the reaction to its surroundings: C₂H₄ + H₂ --> C₂H₆

_{Bond enthalpy}

C=C 300 kJ/mol

H-H 240 kJ/mol

C-H 140 kJ/mol

C-C 136 kJ/mol

• -124 KJ/mol

• 124 KJ/mol

• -2826 KJ/mol

• 2826 KJ/mol

Match the definition below to the correct term.

The enthalpy change that takes place when one mole of a compound is formed from its elements in their standard states under standard conditions.

• The enthalpy of neutralisation

• The enthalpy of combustion

• The enthalpy of formation

• The enthalpy of reaction

What do we mean by the term standard conditions

• 1atm, 20C

• 1atm, 0K

• 10atm, 273K

• 1atm, 298K