Two portions of 50.0 g of water, at 13.0 and 52.0 °C, respectively, were mixed inside a cup calorimeter. If the temperature of water after mixing became 31.0 "C, Calculate the heat capacity of the calorimeter. Given that specific heat of water is 4.184 J/ "C.g. a. 46.5 J/"C b. 69.7 J/"C c. 58.1 J/°C d. 34.9 J/°C De. 23.2 J/°c Clear my choice

[11] A 10.00 g sample of a metal alloy was heated to 88.99 °C. It is then quickly dropped into 40.0 g of water in a calorimeter. The water temperature rises from 19.73 °C to 24.23 °C. Calculate the specific heat of the alloy. [Specific Heat of Water = 4.184 J/g °C and Heat Capacity of Calorimeter = 12.6 J/°C]

2. A solid substance has a mass of 250 grams. It is cooled by 25.00°C and loses 4.937 kJ of heat. What is the specific heat capacity of the substance? 20 3. A 10.0 g sample of pure acetic acid, CH3CO2H, is completely burned. The heat released warms 2.0 L of water from 22.3°C to 39.6°C. I MAR a) Assuming that no heat was lost to the calorimeter, what is the molar enthalpy change of the complete combustion of acetic acid? Express your answer in kJ/mol. b) Will the bonds in the products be longer or shorter than the bonds in the reactants?

The temperature of an object increases by 43.5 °C when it absorbs 3829 J of heat. Calculate the heat capacity of the object. C = The mass of the object is 367 g. Use the table of specific heat values to identify the composition of the object. Substance Specific heat (J/(g. °C)) gold 0.129. silver 0.240 iron 0.444 aluminum 0.900 The object is composed of O aluminum. silver. gold. iron. J/°C

4. The heat capacity of copper is 0.382 J/g°.C. A 22.6 g sample of copper at 93° C is placed in 50 g of water at 23.9° C. What is the final temperature of the system?

Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. How much heat, in J, was absorbed by the water assuming the specific heat of the water is 4.184 J/g･°C?

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?

The specific heat of substance C is 0.93 J/(g K) and that of substance D is 1.8 J/(g K). You are given an unknown that could be pure substance C, pure substance D, or a homogeneous mixture of C and D. In the lab you determine that it requires 23.3 J of heat energy to raise the temperature of a 25.0 g sample of the unknown by 1.0 K. What conclusions can you make about the identity of your unknown, from this data?

An 87.9 g sample of chromium metal at 99.1°C is placed in a calorimeter containing 100.00 g of water at 21.0°C The contents of the calorimeter come to a temperature of 25.7°C. The heat capacity of water is 4.18 J/(g* °C) a. Is this process exothermic or endothermic? b. Calculate the amount of heat released by the metal (q metal) in Joules. Show your work.