SL: When a reaction is endothermic, ΔH is 1 and heat is 2 by the system.

• 1: negative 2: released

• 1: negative 2: absorbed

• 1: positive 2: absorbed

• 1: positive 2: released

Tags

NGSS.HS-PS1-4

SL

• $1072+\left(2\times-296\right)-394$

• $-1072-296-394$

• $-1072+\left(2\times-394\right)+296$

• $\frac{\left(1072-394\right)}{2}+\left(-296\right)$

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

SL

• $38\ kJ$

• $-38\ kJ$

• $0\ kJ$

• $46\ kJ$

Tags

NGSS.HS-PS1-4

SL _____________: the enthalpy change required to break one mole of particular bonds in gaseous molecules.

• enthalpy of formation

• enthalpy of atomisation

• average bond enthalpy

• lattice enthalpy

Tags

NGSS.HS-PS1-4

SL: The standard enthalpy of formation 

( $\Delta H_f^o$  ) of liquid water is zero.

• True

• False

SL: The standard enthalpy of formation 

($$\Delta H_f^o$$ ) of gaseous water is zero.
 

• True

• False

 SL: The standard enthalpy of formation 

($$\Delta H_f^o$$ ) of gaseous  $O_2$   is zero.

• True

• False

Tags

NGSS.HS-PS1-4

HL: The enthalpy change when one mole of gaseous ions is surrounded by water molecules to produce a solution of infinite dilution at 298 K and 100 kPa.

• Standard enthalpy of hydration

• Standard enthalpy of solution

• Lattice enthalpy

• Standard enthalpy of atomisation

The enthalpy change when one mole of an ionic compound is broken into its constituent gaseous ions at 298 K and 100 kPa.

• Standard enthalpy of hydration

• Standard enthalpy of solution

• Lattice enthalpy

• Standard enthalpy of atomisation

Which of the following represents the second ionisation energy of Ca.

• Ca_(s) → Ca²⁺_(g) + 2 e⁻

• Ca_(g) → Ca²⁺_(g) + 2 e⁻

• Ca⁺_(s) → Ca²⁺_(g) + e⁻

• Ca²⁺_(g) + 2 e⁻ → Ca_(s)