Question

Can you please explain to me how to do this question?

$3 Heat and heat trangfer H&T 176 The following two exercises illustrate how the concept of heat transfer can be used to predict the equilibrium temperature of a mixture of hot and cold water Exercise 3.4 we mix 6 g of water at 34°C and 5 g of water at 23°C. The description of the interaction in terms of heat transfer is illustrated at right. Heat A. How much heat must be transferred for the hot water to cool by one degree? In this case, how 5 g 23°C initially 6 g much heat does each gram of cold water receive? 34°C intlly What is the temperature change of the cold water as a whole when the hot water cools one degree? B. Imagine that the same number of calories as in part A is transferred from the hot water to the cold water over and over again until equilibrium is reached. Show the results from each successive transfer of heat in a table like the following: Heat transferred 0 cal Temp. of hot water Temp. of cold water 34°C 33°С 23°C What is the final temperature? What is the total heat transferred?

Answer 1

The amount of heat release by the hot water when it cools down by 1 degree c Q = M_H C_w triangle T_H triangle_H = 1 degree c M_H = 6 g, C_w = 4.186 J/degree c g Q = 6 times 4.186 times 1 = 25.116 J = 6 cal So the heat received by the cold water = 25.116 J = 6 cal Hence each gram of cold water receives each gram leftarroe q = 6/5 = 1.2 cal of heat The change in temperature of the cold water Q = m_c C_w triangle T_c rightdoublearrow triangle T_c = Q/m_c C_w gt rises triangle T_c = 2s.116/s times 4.186 = 1.2 degrees c The change in temperature of the cold water The final temperature = 29 degree c The total heat transferred = 30 cal