6 1 point The amount of heat required to melt 0.02mg of H2O is 12.3J and the amount of heat required to melt 0.16mg of H2O is 36.0J. What type of domain of chemical reaction is this? a. Macroscopic b. Microscopic c. Symbolic microscopic d. Symbolic macroscopic. d a Clear my selection

Why is it a good idea to rinse your thermos bottle with hot water before filling it with hot coffee?

9.29 In which case is heat added to the system: (a) E=43J , w=40J ; or (b) E=31J , w=34J ?

Define the joule in terms of SI base units.

A 0.500-g sample of KCl is added to 50.0 g of water in a calorimeter (Figure 5.12). If the temperature decreases by 1.05 °C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?

What quantity of heat energy must have en applied to a block of aluminum weighing 42.7 g if the temperature of the block of aluminum increased by 15.2 °C? (See Table 10.1.)

9.56 Using heats of formation tabulated in Appendix E, calculate the heats of reaction for the following. (a) C2H2(g)+52O2(g)2CO2(g)+H2O(l) (b) PCl3(g)+Cl2(g)PCl5(g) (c) C2H4(g)+H2O(g)C2H5OH(g) (d) Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(l)

A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5C) to vapor at 59.0C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate H for: Br2(l,22.5C)Br2(l,59.0C) (b) Calculate H for: Br2(l,59.0C)Br2(g,59.0C) (c) Using Hess's law, calculate H for: Br2(l,22.5C)Br2(g,59.0C)

9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)

Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the experimenter used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.