Thermochemistry CP

In the equation q = mcΔT, q stands for the amount of

• energy/heat

• heat capacity

• temperature change

• mass

Tags

NGSS.HS-PS3-4

In the equation q = mcΔT, m stands for the amount of

• energy/heat

• heat capacity

• temperature change

• mass

Tags

CCSS.8.EE.C.7B

In the equation q = mcΔT, c stands for the amount of

• energy/heat

• heat capacity

• temperature change

• mass

Tags

CCSS.8.EE.C.7B

In the equation q = mcΔT, ΔT stands for the

• energy/heat

• heat capacity

• temperature change

• mass

Tags

NGSS.HS-PS3-4

To find ΔT, use

• T_final + T_initial

• T_final - T_initial

• T_{initial -}T_final

• T_{initial x} T_final

Tags

CCSS.8.EE.C.7B

When chemical bonds form, energy is

• released

• required

Tags

NGSS.HS-PS1-4

In order to break chemical bonds, energy is

• released

• required

Tags

NGSS.HS-PS1-4

If overall energy is released in a chemical reaction (feels hot), the reaction is

• endothermic

• exothermic

• isothermic

• hypothermic

Answer explanation

exo = exit

thermic = heat

Tags

NGSS.HS-PS1-4

If overall energy is absorbed in a chemical reaction (feels cold), the reaction is

• endothermic

• exothermic

• isothermic

• hypothermic

Answer explanation

endo = enter

thermic = heat

Tags

NGSS.HS-PS1-4

In an overall chemical reaction, if more energy is needed to break chemical bonds than is released by forming chemical bonds, the reaction is

• endothermic

• exothermic

• isothermic

• hypothermic

Tags

NGSS.HS-PS1-4