time(s) 30 60 120 180 240 300 420 480
t(*c) 13.8 13.8 13.9 13.1 14.2 14.3 14.5 14.7 14.8
b. if t1= 24.5*c, T2= 1.5*C, tr= 23.6*c, and with the tf obtained from the plot, determine Ccal, in J/*C, if the procedure descrived in the laboratory is followed.
3.when 0.600g of metal are added to 100.0mL of 3M HCL, the temperature rose from an initial temperature of 24.1*C to a final temperature of 32.6*C. Calculate the heat of reaction, in kJ/mol of metal, using the information given in the laboratory and assuming the heat capacity of the calorimeter is 32j/*C
b. To determine Ccal, we need to use the information provided in the laboratory. We have the following equations:
t1 = 24.5 * C
T2 = 1.5 * C
tr = 23.6 * C
From the given data, we need to determine the value of tf from the plot. Once we have tf, we can calculate Ccal.
To find tf from the plot:
1. Plot the given data points for time(s) and t(*C) on a graph.
2. Fit a curve through the points to obtain a smooth plot (you can use any suitable curve fitting method).
3. From the plot, locate the corresponding value of tf.
Once we have tf, we can substitute it into the equation T2 = 1.5 * C to solve for C.
3. To calculate the heat of reaction in kJ/mol of metal, we need to use the given information:
Initial temperature (Ti) = 24.1 *C
Final temperature (Tf) = 32.6 *C
Mass of metal (m) = 0.600g
Heat capacity of the calorimeter (Ccal) = 32 J/*C
Molarity of HCl (M) = 3M
The heat of reaction can be calculated using the equation:
q = m * C * ΔT
Where:
q is the heat energy (in J)
m is the mass of the metal (in g)
C is the molar heat capacity (in J/g*°C)
ΔT is the change in temperature (in °C)
To convert q to kJ/mol of metal, we need to convert the mass of the metal to moles using its molar mass (mm):
moles = mass(g) / mm
Then, we can calculate the heat of reaction in kJ/mol of metal:
ΔH = q / moles
Note that the molar mass of the metal is required to perform the conversion from grams to moles.