Sweat cools the body because evaporation is an endothermic process H2O(l) → H2O(g)         ∆H ̊ = +44.01 kJ What mass of water must evaporate from the skin to cool the body by 3.65 ̊C? Assume a body mass of 135 lbs and that the specific heat of the body is 4.00 J/g· ̊C.

The burning of 28g of vegetable cause the temperature of 58.18 g of water in a soda can calorimeter to increase from 21.5°C to 28.1 Calculate the amount of heat absorbed by the water using the specific heat of water at 4.18 J/gºC.

A 12.5-g sample of granite initially at 82.0 °C is immersed into 25.0 g of water that is initially at 22.0 °C. What is the final temperature of both substances when they reach thermal equilibrium? (For water, Cs = 4.18 J/g ⋅ °C and for granite, Cs = 0.790 J/g ⋅ °C.)

You have a sample of water with an unknown amount of mass. You add 348J of heat to the sample and measure the change in temperature to be increasing by 5.2 degrees celsius. What is the mass of the sample of water? The specific heat of water is 4.18 J/(g x degrees Celsius).

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.

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

Evaporating sweat cools the body because evaporation is an endothermic process: H₂O(1)→ H₂O(g) ▲ Hrxn +44.01 kJ = Part A Estimate the mass of water that must evaporate from the skin to cool the body by 1.20 °C. Assume a body mass of 85.0 kg and assume that the specific heat capacity of the body is 4.00 J/g ° C. Express your answer in grams to three significant figures. m = VE ΑΣΦ ? 8.0 g

When a sample of titanium was supplied 1.00 kJ of energy, the temperature rose 103.5 °C. If the specific heat of titanium is 0.523 J/g · °C, what is the mass of the titanium sample?

A student reacts 2.0 moles A and 4.0 moles of B in an insulated container. The reaction takes place in water (50.0 g), in a coffee cup. The water gains heat, raising its temperature 23.6°C (AT). Water has a specific heat capacity of 4.184 J/g C. A + 2B 3 C AHRXN = ? 1 a. Energy is absorbed by the water. What is qWATER? b. Energy is released by the reaction. What is qRXN? (this one is easy) c. How much heat per mol of A (or per 2 mol of B), by the reaction (AHRXN)? d. In another reaction, a student reacts 15.2 moles of B with excess A. What is the heat that comes out of his second reaction (qRXN-2)? use dimensional analysis +

A 29.41 gram piece of metal (specific heat, 0.51 J/g•°C) with an initial temperature of 46.2°C is added to 289.35 grams of water (specific heat, 4.184 J/g•°C) initially at 36.4°C. If the final temperature of the system is 49.8°C, how much heat (in joules) was transfered into the water?