Unit 8 AP Chemistry

The diagram represents which type of reaction

• endothermic

• exothermic

Tags

NGSS.HS-PS1-4

For the reaction 2H₂(g) + O₂(g) → 2H₂O(g) the bond enthalpies (in kJ/mol) are H-H = x, O=O = y, O-H = z Which calculation will give the value, in kJ/mol, of ΔH for the reaction?

• 2x + y - 2z

• 4z - 2x - y

• 2x + y - 4z

• 2z - 2x - y

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

Calculate the change in Gibbs free energy for each set of ΔH°rxn, ΔS°rxn, and T. (Assume that all reactants and products are in their standard states.)

ΔH°rxn = −119 kJ ; ΔS°rxn = +242 J/K ; T = 308 K
Express your answer in kilojoules to three significant figures.

ΔG°rxn = ___ kJ

Select the orbital.

Tags

NGSS.HS-PS1-1

Select the electron.

Tags

NGSS.MS-PS1-1

Select the subatomic particle that has a mass of 1 AMU.

Tags

NGSS.MS-PS1-1

NGSS.MS-PS1-5

Calculate the change in Gibbs free energy for each set of ΔH°rxn, ΔS°rxn, and T. (Assume that all reactants and products are in their standard states.) ΔH°rxn = −119 kJ ; ΔS°rxn = −242 J/K ; T = 308 K Express your answer in kilojoules to three significant figures. ΔG°rxn = ___ kJ

Tags

NGSS.HS-PS3-1

Calculate the standard entropy change for the following reaction: Cu(s)+1/2 O₂(g) → CuO(s). Given that S⁰ (Cu(s)) = 33.15 J/K*mol S⁰ (O₂(g)) = 205.14 J/K*mol S⁰ (CuO(s)) = 42.5 J/K*mol

• 195.66 J/K.mol

• 93.09 J/K.mol

• -93.09 J/K.mol

• +195.66 J/K.mol

Tags

NGSS.HS-PS3-4

Energy is required to ________bonds.

• form

• break

Tags

NGSS.HS-PS1-4