An experiment was conducted to determine the specific heat of platinum. It was determined that 158.8 Joules of heat were required to increase the temperature of a 50.0 gram sample of platinum from 20.0 °C to 45.5 °C. Based on these experimental results calculate the specific heat (J/g.°C) of platinum. Do not type units into your answer.

A sample of copper absorbs 44 kJ of heat, resulting in a temperature rise of 65 °C. Determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.

A hot 105.9 g lump of an unknown substance initially at 154.0 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 36.2 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. rhodium ○ graphite titanium zinc tungsten aluminum Substance Specific heat (J/(g∙°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 tungsten 0.132 zinc 0.388 water 4.184

An experiment was conducted to determine the specific heat of platinum.  It was determined that 158.8 Joules of heat were required to increase the temperature of a 50.0 gram sample of platinum from 20.0 oC to 45.5 oC.  Based on these experimental results calculate the specific heat (J/goC) of platinum.  Do not type units into your answer.

The specific heat of lead is 0.128 J/g·°C. How much heat is needed to raise the temperature of 4.90 g of lead by 46.0 °C?

A 30.0g piece of copper absorbs 481.95 J of heat while rising from 23.0°C to 65.5 °C. Calculate the specific heat of copper.

A chemist carefully measures the amount of heat needed to raise the temperature of a 744.0 mg sample of a pure substance from -7.8 °C to 12.8 °C. The experiment shows that 3.60 J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.

In the laboratory a student determines the specific heat of a metal.He heats 18.4 grams of platinum to 99.28 °C and then drops it into an insulated cup containing 85.3 grams of water at 23.56 °C. When thermal equilibrium is reached, he measures the final temperature to be 24.10 °C.Assuming that all of the heat is transferred to the water, he calculates the specific heat of platinum to be  J/g°C.

You discover a new substance and wish to determine its specific heat capacity. Your sample weighs 229 g and upon absorbing 16.4 kJ of heat the temperature is raised from 19.6K to 53.7K. What is the specific heat capacity (in J/g•K) of the metal?

An experiment was conducted to determine the specific heat of platinum.  It was determined that 158.8 Joules of heat were required to increase the temperature of a 50.0 gram sample of platinum from 20.0 oC to 45.5 oC.  Based on these experimental results calculate the specific heat (J/g⋅⋅oC) of platinum.