The goal of this pod is to solve problems
in which you are looking for final temperature or initial temperature of
an object.
These are a little bit more algebraically difficult than solving for other variables.
To these problems,
it can be helpful to use a different version of the formula.
$$
Q = m c \Delta T \; \; \; \; \; \; \; \; \; \; Q = m c \left( T_f  T_i \right)
$$
\( Q \)
Heat Energy Transferred
Joules (J)
\( m \)
mass
kilograms (kg)
\( c \)
Specific Heat of Substance
\( \frac{ \text{J} }{ \text{kg} \cdot ^{\circ} \text{C} } \)
\( T_f \)
Final Temperature
Kelvin (K) or Degrees Celsius (\( ^{\circ} \text{C} \))
\( T_i \)
Initial Temperature
Kelvin (K) or Degrees Celsius (\( ^{\circ} \text{C} \))
Material
Specific heat \( \left( \frac{ \text{J} }{ \text{kg} \cdot ^{\circ} \text{C} } \right) \)

I have 0.800 kg of water with a temperature of 30.0°C.
I add 10,000. Joules of energy to the water.
What will be the final temperature?

A gold ring has a temperature of 22°C
and a mass of 200 grams.
If a metal worker adds 5624 Joules of heat energy to the ring,
what is its final temperature?

A massive concrete building has a temperature of 5°C
and a mass of 4000 kilograms at night.
The sun rises and adds \( 6.69 \cdot 10^7 \) Joules of heat energy
to the building.
What is its final temperature?

Somebody heats a bowl of 3 kg of water
to its boiling point (100°C) by adding
941400 Joules of heat energy.
What was its initial temperature?

By rubbing wooden sticks together,
somebody adds 7560 Joules of heat energy.
The sticks have a mass of 0.200 kg,
and they reach a final temperature of 35°C.
What was their initial temperature?

Someone has been cooking with a hot pot, but after taking
it off the heat it returns to room temperature.
The pot is mostly steel and has a mass of 0.85 kg.
It gives off 47141 Joules of heat energy
when it reduces its temperature of 22°C.
What was its initial temperature?