#14 - Endo/Exo, Scientific Notation, Enthalpy, & Q=mCΔT

Categorize these properties of endothermic and exothermic reactions:

Temperature is a measurement of the ​​ (a)   of the molecules inside a substance.

The ​ (b)   a substance is, the ​ (c)   the particles move, and the greater the ​kinetic energy.

The ​ (d)   a substance is, the ​ (e)   the particles move, and the lower the kinetic energy.

Match the number in standard form to it's equality in scientific notation:

If you use 12 g of water in a reaction that releases 1250 J of energy, what is the ΔT?

Q = ​ (a)  

m = ​ (b)  

C = ​ (c)  

ΔT = ​ (d)  

If you use 5 g of water in a reaction that has an initial temperature of 22.4°C and a final temperature of 45.8°C, how much energy was absorbed?

Q = ​ ​ (a)  

m = ​ (b)  

C = ​ (c)  

ΔT = ​ (d)  

If a reaction releases 57,000 J of energy and has an initial temperature of 22.4°C and a final temperature of 5.8°C, what was the mass of the water?

Q = ​ ​​ (a)  

m = ​ ​ (b)  

C = ​ (c)  

ΔT = ​​ (d)  

If a reaction has a mass of 13 g, absorbs 1,500 J of energy, has an initial temperature of 22.4°C, and a final temperature of 34.7°C, what is the specific heat capacity of the substance?

Q = ​ ​​ (a)  

m = ​ ​ (b)  

C = ​ (c)  

ΔT = ​​​ (d)  

Label the chemical equations and graphs correctly:

Calculate the enthalpy of both graphs:

When the change in enthalpy (ΔH) is positive, the reaction is ​​ (a)   . When the change in enthalpy (ΔH) is negative, the reaction is ​​ (b)   . In an exothermic reaction, energy moves from ​the ​ (c)   to the ​ (d)   . A chemical reaction that ​ (e)   heat is called an ​endothermic reaction.