AP Chemistry Unit 6 Review

Calculate the value of  $\Delta E$  in joules for a system that loses 50 J of heat and has 150 J of work performed on it by the surroundings

• +200

• -100

• 100

• -200

• 50

Tags

NGSS.HS-PS3-1

The value of  $\Delta H\degree$  for the reaction below is -126 kJ. _____ kJ are released when 2.00 mol of NaOH is formed in the reaction?

• 63

• 252

• 3.9

• -126

• 7.8

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

The value of  $\Delta H\degree$  for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ____ kJ.

• -12

• -790

• -23

• 23

• 12

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

The value of  $\Delta H\degree$  for the reaction below is +128.1 kJ. How many kJ of heat are consumed when 5.10 g of  $H_2$   (g) is formed as shown in the equation?

• 653

• 326

• 162

• 128

• 62.0

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-4

 $\degree$ The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 $\degree$  C to 37 $\degree C$  .

 

• 0.00054

• 29

• 0.13

• -0.13

• 2.0

Tags

NGSS.HS-PS3-4

The specific heat of bromine liquid is 0.226 J/g-K. The molar heat capacity (in J/mol-K) of bromine liquid is ____.

• 707

• 0.226

• 9.05

• 36.1

• 18.1

 $\degree$  The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the temperature of 10.0 mL of bromine from 25.00 $\degree C$  to 27.30  $\degree C$  ? The density of liquid bromine: 3.12 g/mL.

• 5.20

• 16.2

• 32.4

• 10.4

• 300

Tags

NGSS.HS-PS3-4

Given the data in the table above,  $\Delta H_{rxn}\degree$  for the reaction is ______ kJ.

• -1892

• -1172

• -150

• -1540

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

Given the data in the table above,  $\Delta H\degree_{rxn}$  for the reaction is _____________ kJ.

• -3.2

• -1.6

• 1.6

• 3.2

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

 $\Delta H$  for the reaction is ____ kJ.

• -1135

• 1135

• 35

• -35

• 355

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1