# Calorimetry Lab

Topics: Temperature, Absolute zero, Heat Pages: 4 (1387 words) Published: June 14, 2011
Calorimetry
To determine the specific heat of a metal and its approximate atomic mass. To determine the heat of neutralization for a strong acid-strong base reaction. To determine the quantity and direction of heat flow for the dissolution of salt.

1.In parts A and B in, the calorimeter, although a good insulator, absorbs some heat when the system is above room temperature. Is the reported value for the specific heat of the metal too high or too low? Explain. Is the reported DeltaHn value for the acid- base reaction too high or too low? Explain. The DeltaHn value reported in Part B will be lower than the true value because the true Delta T will never be reached. Since the calorimeter absorbs some heat when the system is above room temperature the DeltaT will be too low. Since DeltaT is too low, q in q=mc DeltaT equation will be too low. Therefore, DeltaH is too low. 2.The DeltaHn value for the two strong acid-strong base reactions should be the same, within experimental error. Explain. The DeltaHn values for the two strong acid-strong bases reactions should be the same, within experimental error, because the net ionic equations are the same for both reactions. 3.If you use a thermometer that is miscalibrated to read .4 degrees Celsius higher over its entire range, does this affect the value for DeltaHn? Explain. If a thermometer is miscalibrated to read .4 degrees Celsius higher over its entire range the DeltaHn value will be unaffected because the DeltaT will be unchanged due to the miscalibration. 4.If the maximum recorded temperature is used in Part B, rather that the extrapolated temperature, will be reported DeltaHn be higher or lower than the accepted value? Explain. If the maximum recorded temperature is used in Part B, rather that the extrapolated temperature, DeltaHn will be too small. This is due to the fact that the maximum temperature is lower than the temperature of the...