The specific heat of iron is 0.449 J/(g) (°C). Calculate the energy (in J) absorbed if the temperature changed from 30 °C to 100°C and the mass of the iron is 100g *

The specific heat capacity of solid iodine is 0.427 J/g⋅⋅oC.  Calculate the final temperature (°C) when 747.0 J of heat is added to a 186.5g sample of solid iodine initially at 13.3°C. Please use the correct significant digit   I got my answer as 22.3; however, it is incorrect. I am a bit lost on why.

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 38.7 °C. During the reaction 55.6 kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is -1 4.18 J∙g¯¹·K¯¹. Be sure your answer has the correct number of significant digits. 心。 °℃ x10 S

A gas expands and does work on the surroundings equal to 4.92 Latm. At the same time, it releases 98.6 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)

How many grams of an unknown substance, having a specific heat of 1.66 J g ° C, are present if a temperature change of -173.4 K occurs. The heat lost was 35981 J.

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 3.40kg of water at 32.4°C. During the reaction 60.8kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g−1K−1. Be sure your answer has the correct number of significant digits.

Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. How much heat, in J, was absorbed by the water assuming the specific heat of the water is 4.184 J/g･°C?

In the laboratory a student finds that it takes 145 Joules to increase the temperature of 14.7 grams of solid silicon from 23.0 to 38.0 degrees Celsius. The specific heat of silicon calculated from her data is J/g°C.

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A student heats 62.45 grams of platinum to 99.18 °C and then drops it into a cup containing 84.71 grams of water at 23.23 °C. She measures the final temperature to be 25.02 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.66 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of platinum.