The table provides molar heat capacities (Cm) of selected Molar heat capacity (Cm) of selected metals metals with the units of joules per mole-kelvin. Heat capacity is also frequently given as specific heat capacity ( at 25 °C Element Cm (J/(mol·K)) C,) with the units joules per gram-degree Celsius. aluminum 24.20 Using the values provided in the table, convert the molar copper 24.44 heat capacity (Cm) of magnesium to the specific heat iron 25.10 capacity (C,) of magnesium. lead 26.84 magnesium 24.87 nickel 26.07 titanium 25.06 zinc 25.39 C; = J/(g · °C)

The table provides molar heat capacities (Cm) of selected Molar heat capacity (Cm) of selected metals metals with the units of joules per mole-kelvin. Heat capacity is also frequently given as specific heat capacity ( at 25 °C Element Cm (J/(mol·K)) C,) with the units joules per gram-degree Celsius. aluminum 24.20 Using the values provided in the table, convert the molar copper 24.44 heat capacity (Cm) of magnesium to the specific heat iron 25.10 capacity (C,) of magnesium. lead 26.84 magnesium 24.87 nickel 26.07 titanium 25.06 zinc 25.39 C; = J/(g · °C)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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5c
Suppose 200.0 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH, both initially at 25.0°C, are mixed in a thermos flask. When the reaction is complete, the temperature is 28.4°C. Assuming that the solutions have the same heat capacity as pure water, compute the heat released (in kJ).
Calcium carbonate can be decomposed upon applying heat with the following equation CaCO3(s) → CaO(s) + CO2(g) ΔH = +179.5kJ How much heat will be needed to decompose 30 g of calcium carbonate? AND What size container will be required (in L) to contain the carbon dioxide generated at 25ºC and 1.2 atm?
Suppose 300 mL of 2.00 M HCl and 300 mL of 2.00 M NaOH, both initially at 23.0 celsius, are mixed in a thermos flask. When the reaction is complete, the temperature is 36.6 celsius. Assuming that the solutions have the same heat capacity as pure water, compute the heat released in kJ
A piece of metal of mass 15 g at 99◦C is placed in a calorimeter containing 41.3 g of water at 19◦C. The final temperature of the mixture is 40.2◦C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings. Answer in units ofJg·◦C.
Iron can be extracted from the iron(III) oxide found in iron ores (such as haematite) via an oxidation-reduction reaction with carbon. The thermochemical equation for this process is: 2 Fe203(s) + 3 C(s) → 4 Fe(1) + 3 CO2(g) AH° = +467.9 kJ
The table provides molar heat capacities (Cm) of selected metals with the units of joules per mole-kelvin. Heat capacity is also frequently given as specific heat capacity (C₂) with the units joules per gram-degree Celsius. Using the values provided in the table, convert the molar heat capacity (Cm) of zinc to the specific heat capacity (C₂) of zinc. C₁ = J/(g. °C) Molar heat capacity (Cm) of selected metals at 25 °C Element aluminum copper iron lead magnesium nickel titanium zinc Cm (J/(mol-K)) 24.20 24.44 25.10 26.84 24.87 26.07 25.06 25.39
Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction: 2Al(s) + Fe203(s) → Al203(s) + 2Fe(s) This reaction occurs when a mixture of powdered aluminum and iron(III) oxide is ignited with a magnesium fuse. The following enthalpies of formation are known: AH°; for Fe203(s) = -826 kJ AH°; for Al203(s) = -1676 kJ O 1251 kJ O 2502 kJ O-1251 kJ O 425 kJ 850 kJ O- 2502 kJ -850 kJ -425 kJ
Measurements show that the enthalpy of a mixture of gaseous reactants increases by 195.kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 69.kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. Is the reaction exothermic or endothermic?
When a 45.0 g sample of an alloy at 100.0 °C is dropped into 55.0 g of water at 25.0 °C, the final temperature is 30.4 °C. What is the specific heat of the alloy? The specific heat of H2O(l) is 4.184 J·g–1·°C–1. (A) 0.397 J·g–1·°C–1. (B) 0.447 J·g–1·°C–1. (C) 1.28 J·g–1·°C–1. (D) 1.55 J·g–1·°C–1.
A block of iron weighing 4.50 kg at a temperature of 107.0 °C was inserted into a container containing 1.2 liter of water at a temperature of 30.0 °C isolated from the environment. What is the final temperature (in °C) of the water and the iron at the end of the process? (The specific heat of solid iron is 0.450 J lg .r and the specific heat of water is 4.184 J/ g°C) Density of water = 1.0 g/mL.