The temperature of a sample of iron increased by 23.4 °C Substance Specific heat J/(g °C) when 269 J of heat was applied. lead 0.128 What is the mass of the sample? silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 m =

The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 0.385 0.449 0.903 4.184 copper iron aluminum water An unknown substance has a mass of 18.9 g. The temperature of the substance increases by 16.5 °C when 73.3 J of heat is added to the substance. What is the most likely identity of the substance? water Olead O copper iron. silver aluminum

A 234.66 gram aqueous solution has a specific heat of 4.186 J/gºC. The solution is at 28.1 °C. What is the temperature of the solution in °C after 54.93 kJ of heat has been added to it?

The temperature of the solution increases from 21.3 °C to 38.2 °C. 0.468 g Mg reacting0.0193 mol Mg reacting80.844 g HCl solution The energy released is given by q = specific heat × mass × temperature changeThe solution is almost all water, so we use the specific heat capacity of water, 4.18 J/g•°C. What is the quantity of heat released? Enter your answer as a positive value.

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)

What is the specific heat of a 45.51 g piece of an unknown metal that exhibits a 45.2 °C temperature change upon absorbing 1870 J of heat?

IT The temperature of a sample of aluminum increased by 24.6 °C when 255 J of heat was applied. Substance Specific heat J/(g lead 0.128 What is the mass of the sample? silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 m =

Which of the reactions are exothermic? 2 Mg(s) + O,(g) → 2 MgO(s) + heat O NH, (g) + HCI(g) → NH,CI(s) + heat AgCl(s) + heat – Ag*(aq) + Cl¯(aq) 2 Fe, 0, (s) + 3 C(s) + heat → 4Fe(s) + 3 CO, (g) O C(graphite) + 0,(g) → CO,(g) + heat O CH, (g) + 20,(g) → CO,(g) + 2 H,O(1) + heat

A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C.   If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt?   How many moles of the unknown salt were used in the reaction ?     _______ J?