3)
Given:
m = 122 g
C = 0.451 J/g.oC
Ti = -11.2 oC
Tf = 33.5 oC
use:
Q = m*C*(Tf-Ti)
Q = 122.0*0.451*(33.5--11.2)
Q = 2459 J
Answer: 2.46*10^3 J
Only 1 question at a time please
How much heat is released from a 500 g iron rod when it cools from 125°C to 20°C? The specific heat of Fe is 0.451 J/gºC
please help?
How much heat is released from a 500 g iron rod when it cools from 125°C to 20°C? The specific heat of Fe is 0.451 J/gºC O-23678J 10.6J O-32698 O 23.7J
Use the heat equation to calculate the energy, in joules and calories, for each of the following (see the table): Specific Heats for Some Substances Substance cal/g ∘Ccal/g ∘C J/g ∘CJ/g ∘C Elements Aluminum, Al(s)Al(s) 0.214 0.897 Copper, Cu(s)Cu(s) 0.0920 0.385 Gold, Au(s)Au(s) 0.0308 0.129 Iron, Fe(s)Fe(s) 0.108 0.452 Silver, Ag(s)Ag(s) 0.0562 0.235 Titanium, Ti(s)Ti(s) 0.125 0.523 Compounds Ammonia, NH3(s)NH3(s) 0.488 2.04 Ethanol, C2H6O(s)C2H6O(s) 0.588 2.46 Sodium chloride, NaCl(s)NaCl(s) 0.207 0.864 Water, H2O(s)H2O(s) 1.00 4.184 Water, H2O(s)H2O(s) 0.485 2.03 a.)...
How much heat is released when 150. g of iron cools from 525°C to 100°C? (Cp = 0.44 J/gºC) A 50.0 g block of glass (Cp = 0.50 J/gºC) absorbs 333 joules of heat energy. How much does the temperature of the glass rise? The temperature of a silver coin (Cp = 0.24 3/9°C) falls by 353 °C as it releases 5,550 Joules of heat. What is the mass of the coin 5.
4. Heat transfer: q = mass x Cs x ΔT and –qreaction = +qsolution a. A piece of metal with a mass of 8.6 g was heated to 100.0°C and dropped into a coffee cup calorimeter containing 402.4 g of water at 25.0°C. If the temperature of the water and the metal at thermal equilibrium is 26.4°C, what is the specific heat of this metal in J/g°C? b. How much heat energy must be added in order to boil a...
the Specific Heat Capicity of Tungsten is given here.
3. Calculate the temperature change when 32 grams of tungsten has 21 Joules of heat added to it. temperature be- in between the initial temperatures of the t and will be the same for the metal and the water.) Table 1. Specific heat capacities of various metals and other substances Specific Heat Capacity, C (J/g.°C) 0.129 0.129 0.132 0.133 Specific Heat Capacity, C (3/goC) 0.421 0.444 0.449 0.450 0.460 0.522 0.757...
How much heat, in J (Joules), is required to warm 32.1 g of water from 20.1 ∘C to 63.1 ∘C?
How much heat must be removed from 456 g of water at 25.0 degree C to change it into ice at -10.0 degree C? The specific heat of ice is 2090 J/kg K. the latent heat of fusion of water is 33.5 times 10^4 J/Kg, and the specific heat of water is 4186 J/kg K.
A. How much heat energy, in kilojoules, is required to convert 68.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to three significant figures and include the appropriate units. B. How long would it take for 1.50 mol of water at 100.0 ∘C to be converted completely into steam if heat were added at a constant rate of 17.0 J/s ? Express your answer to three significant figures and include the appropriate units.
Be sure to answer all parts. How much heat has to be added to 251 g of iron at 25.0°C to raise the temperature of the iron to 250.0° C? (The specific heat of iron is 0.448 J/g °C.) Prev 15 of 17 !! Next >