The next several questions are all for one problem of putting a hot piece of metal into a coffee cup of cold water and finding the final temperature. The equation that will be used starts with –q(hot) = q(cold). Which says the coffee cup does not absorb heat, and the heat lost by the hot metal is equal in magnitude, and opposite in sign, to the heat gained by the cold water. Each of these q will be replaced with what? Select one: a. the mass times the specific heat capacity times the final temperature b. the mass of the object c. the mass times the specific heat capacity times the initial temperature d. none of these e. the mass times the specific heat capacity times the change in temperature f. the mass times the specific heat capacity

A 27-gram piece of metal at 144  oC is dropped into 86 grams of water at 29 oC.  The water temperature rose to 37 oC.  Calculate the heat change of the metal in Joules.  (DO NOT PUT UNITS IN YOUR ANSWER.)  Assume that all of the heat lost by the metal is transferred to the water and no heat is lost to the surroundings.  The specific heat of water is 4.184 J / g oC.

Suppose that the reaction of 3.49 moles produces 1.46 kJ of heat. What is the molar enthalpy of the reaction in kJ/mol? Report your answer to three decimal places (ignore significant figures).

10. Ethanol OH weighing 3.56 g is burned in a calorimeter. The temperature rises from 15.C to C. The temperature rises from 15.1 If to 28. heat of the bomb plus water is 8.224C. Find the Δ in kJ/mol.  (provide the given and required to find in the problem) (Kindly provide a CLEAR and COMPLETE solution) (Answer should be typewritten)

What is the volume in L required to heat the water?

Rachel West Section 017 A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as ie reaction proceeds. Is this reaction endorhermic or exothermic? Describe if heat energy is lost or gained Trom the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the cemperature of the surrounding solution increase or decrease as a result of this chemical process?

Suppose object A has quadruple the specific heat and double the mass of object B. If the same amount of heat is applied to both objects, how will the temperature change of A be related to the temperature change of B? Enter your answer to three significant figures. Temperature change of A = i × (temperature change of B)

Please help me complete this question

2 moles of lithium metal reacts with liquid water to produce solid lithium hydroxide, hydrogen gas, and 402.4 kJ/mol of heat energy. a) write a balanced thermochemical equation for the reaction b) how much heat would be produced by the reaction of 14 g of lithium with an excess of liquid water  c) is the reaction endothermic or exothermic?

What mass of water will change its temperature by 10 °C when 975 J of heat is added? The specific heat of water is 4.18 J/g 0C