Question

A sample of silver is heated from 1,972.36 degrees C until it is completely boiled (converted from a liquid to a gas) at its boiling point 2,162 degrees C.  If the sample has a mass of 96.68g, how much total energy, in joules, was transferred into the silver?

Answer 1

The total energy is 4345.25 J

Step-by-step explanation

From the question, we have the following given data

`\begin{gathered} \text{Initial temperature, T}_1=1972.36\text{ degr}ees\text{ C} \\ \text{Final }temperature,T_2\text{ = 2162 degr}ees\text{ C} \\ \text{Mass of silver, m = 96.68 g} \end{gathered}`

Since the specific heat of silver is 0.237 J/g°C. Therefore the formula to calculate the total energy transferred will be

`\begin{gathered} q=mc\Delta T \\ q\text{ is the total energy in joules} \\ m\text{ is the mass of silver in gram = 96.68 g} \\ c\text{ is the specific heat of silver J/g degre}e\text{ C = 0.237 J/g}^0C \\ \Delta T\text{ is the temperature rise in degr}ees\text{ celcius} \\ \Delta T=T_2-T_1=2162-1972.36=189.64^0C \\ \Rightarrow q=96.68*0.237*189.64 \\ q=4345.25\text{ joules} \end{gathered}`