The heat of combustion of isobutane, CH(CH3)3, is -2869. kJ/mol of isobutane. If a calorimeter indicates 64.7 kJ of heat was released, what is the mass in grams of carbon dioxide that has been produced in the combustion of a sample of isobutane? Provide your answer with the appropriate number of significant figures.

A student is asked to identify an unknown piece of metal. The metal has a mass of 12.34 g. It is placed in a boiling water bath and brought up to 99.98 oC. A coffee-cup calorimeter is set up with 103.25 mL of water (density = 1.00 g/mL and specific heat = 4.184 J/g.oC) at a room temperature of 21.30 oC. The metal is removed from the boiling water and placed in the calorimeter. A final temperature is recorded as 22.32 oC. Find the specific heatcapacity of the unknown metal. (Assume there is no heat loss)

Calculate the heat of reaction (in J)

The specific heat capacity of silver is 0.2386 J/g °C. Assuming no loss of heat to the surroundings or to the calorimeter, determine the final temperature when 100.0 g of silver at 40.0°C is immersed in 60.0 g of water at 10.0°C.

Expressing amounts of energy in different energy units is necessary to solve many chemistry problems. For practice, complete the following table. The Joule (J) is the SI unit of energy. 1 calorie (cal) = 4.184 J J cal kJ 549       197       0.806

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 8.40 kg of water at 25.0 °C. During the reaction 97.5 kJ of heat flows out of the flask and into the bath. - 1 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 ·K'. Round your answer to 3 significant digits. x10 ?

The specific heat of aluminum is 0.897 J/g·°C and the specific heat of water is 4.18 J/g·°C.  If a 3.00 g piece of aluminum at 300.0°C is immersed in 10.0 mL of water at 30.0°C, predict the final temperature of the mixture.

In the following reaction, how many grams of CH3OH are required to produce 1.578 x 10° kJ of heat? 2 CH3OH (1) +3 O2 (g) → 2 CO2 (g) + 4 H2O(g) AH = -1280. kJ/mol Please do not include units in your answer.

1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?

A calorimeter is charged with 59.197 mL of water at 24.2 °C. After a reaction takes place in the calorimeter, the water temperature is 25.2 °C. How much heat did the reaction produce, and was it exothermic or endothermic? (The density of water is 1.00 g/mL.)