5.00 kg of some liquid at 10.0 $\circ$ C is mixed with 1.00 kg of the same liquid at 40.0 $\circ$ C.What is the final equilibrium temperature? Ignore any heat flow with the containers and/or surroundings.

Question

Quizplus · Accepted Answer

By using the principle of conservation of energy, we can write:
(mass of liquid 1) x (specific heat capacity of liquid 1) x (change in temperature of liquid 1) = (mass of liquid 2) x (specific heat capacity of liquid 2) x (change in temperature of liquid 2)
Plugging in the values given:
(5.00 kg) x (specific heat capacity) x (final temperature - 10.0C) = (1.00 kg) x (specific heat capacity) x (40.0C - final temperature)
Simplifying and solving for final temperature:
28.0C x 5.00 =  (40.0C - final temperature) 
140.0C =  40.0C - final temperature
Final temperature = 15.0C or 15.0F1F1F1S1F1F1F10C. Therefore, the answer is B.

500 Kg of Some Liquid at 10 ∘\circ∘ C Is Mixed with 1

500 Kg of Some Liquid at 10 $\circ$ C Is Mixed with 1