Let the formula of the metal chloride be MClx
As per Dulong's Petits law,
specific heat*atomic mass of the metal = 25
thus, atomic mass of the metal = 65.79 g/mole
Now, moles of metal in 0.5007 g of it = mass/molar mass = 0.5007/65.79 = 0.0076
mass of Cl in the metal chloride = 1.0586 - 0.5007 = 0.5579
Thus, moles of Cl in the chloride sample = 0.5579/35.5 = 0.0157
Thus, M & Cl are present in the molar ratio of 0.0076:0.0157 = 1:2
Thus, the formula of the compound is MCl2
Now, moles of M in the compound = (1/2)*moles of Cl = (1/2)*0.0157 = 0.00785
Thus, molar mass of M = mass/moles = 0.5007/0.00785 = 63.78 g/mole
The specific heat of a metal was found to be 0.38 J/g. Degree C. When 0.5007...
Calculate the specific heat (J/g degree C) for each of the following: a. a 13.5-g sample of zinc (Zn) heated from 24.2 degree C to 83.6 degree C that absorbs 312 J of heat b. a 48.2-g sample of a metal that absorbs 345 J with a temperature increase from 35.0 degree C to 57.9 degree C
A 130.0 g piece of copper (specific heat 0.38 J/g・°C) is heated and then placed into 400.0 g of water initially at 20.7°C. The water increases in temperature to 22.2°C. What is the initial temperature of the copper? (The specific heat of water is 4.18 J/g・°C and the density of water is 1.00 g/mL).
What is the specific heat of a metal (in j/g degree C) which has a mass of 126.0 grams and requires 1000 joules of heat energy to increase its temperature from 25.0 degree C to 76.0 degree C?
In problems I, II, and III: Calorimeter constant is 0.00 j/degree C Specific Heat of water or aqueous solutions is 4.18 j/g degree C I. 76.9619 g of metal were heated to 100.7 degree C and poured into a calorimeter containing 46.30 g of water at 25.00 degree C. After stirring, the temperature of the water rose rapidly to 32.40 degree C before slowly starting to fall. Calculate: a) The Specific Heat of the metal b) The Atomic Weight Calculated...
Question 10 of 20 A 141.9 g piece of copper (specific heat 0.38 J/g.°C) is heated and then placed into 400.0 g of water initially at 20.7°C. The water increases in temperature to 22.2°C. What is the initial temperature of the copper? (The specific heat of water is 4.18 J/g °C).
Table 1. Selected Properties of Some Metals Atomic Mass Specific Heat (J/g°C) Color or Metal Density (g/mol) Appearance Magnesium 24.31 1.02 Shiny gray metallic 1.738 g/cm Aluminum 26.98 0.90 Silvery gray metallic 2.70 g/cm Nickel 58.69 0.44 Silver, gold tinge metallic 8.908 g/cm Copper 63.55 0.38 Lustrous red-orange 8.96 g/cm Zinc 65.38 0.51 Silver-gray metallic 7.14 g/cm 107.87 Shiny white metallic 10.49 g/cm Silver 0.24 Gold 196.87 0.13 Metallic yellow 19.30 g/cm 9.78 g/cm 0.12 Lustrous brownish silver Bismuth 208.98...
A piece of metal with a specific heat of 1.29 J/g°C is heated to 126.6°C and then placed in 133.868 g of water which is at a temperature of 10.9 °C. After a minute, the temperature of the water has stopped changing and is now 45.6°C. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/g°C. Enter...
A 29.3 g piece of metal is heated to 97 degree C and dropped into a calorimeter containing 50.0 g of water (specific heat capacity of water is 4.18 J/g degree C) initially at 22.9 degree C. The empty calorimeter has a heat capacity of 125 J/K. the final temperature of the water is 25.96 degree C. Ignoring significant figures., calculate the specific heat of the metal. A) 0.481 J/gK. B) 0.361 J/gK C) 0.120 J/gK D) 0.300 J/gK E)...
What is the specific heat (J/g•°C) of a metal object whose temperature increases from 82°C to 147°C when 15.2 g of metal was heated with 45.0 J? Jlg. *C
A 95.0g piece of metal (with a specific heat of 1.55 J/g°C) is
heated to 375°C and then placed into a calorimeter, which contains
60.0g of ice in equilibrium with 40.0g of liquid water. How many
grams of ice will melt in this process? A) 7.3, B) 16.6, C) 34.2,
D) 22.9, or E) 52.4. [The key says the answer is B]. Please show all work. Thank
you!
9. A 95.0 g piece of metal (with a specific heat of...