980000/ (6200*4.180)+18`c or 291K
final answer should be 56`c or 329K.
The metal with the lowest thermal capacity.
21
When hot metal is added into the water then the metal looses its energy into the water and this heat is gained by the water, so the temperature gets increases when hot metal added into it i.e final temperature is greater than initial temperature of water.
When allowed to stand for long enough, the final temperature will reach room temperature.
When allowed to stand for long enough, the final temperature will reach room temperature.
The metal with the lowest thermal capacity.
21
When hot metal is added into the water then the metal looses its energy into the water and this heat is gained by the water, so the temperature gets increases when hot metal added into it i.e final temperature is greater than initial temperature of water.
As an object is heated, the rate of increase in temperature is proportional to the rate of heat added. The proportionality is called the heat capacity. Because the heat capacity is actually a function of temperature in real materials, the total amount of energy added will be equal to the integral of the heat capacity function over the interval from the initial temperature to the final temperature. If you just assume an average heat capacity over the temperature range, then the rise in temperature will be exactly proportional to the amount of heat added.
As an object is heated, the rate of increase in temperature is proportional to the rate of heat added. The proportionality is called the heat capacity. Because the heat capacity is actually a function of temperature in real materials, the total amount of energy added will be equal to the integral of the heat capacity function over the interval from the initial temperature to the final temperature. If you just assume an average heat capacity over the temperature range, then the rise in temperature will be exactly proportional to the amount of heat added.
This depends on the volume.
if 2.5kg of hot water at 100c is added to 10kg of cold water at 28c and stirred well. what is the final temperature of mixture? (neglect the heat absorbed by container and the heat lost by the surroundings.)
q( enthalpy of heat in Joules-energy ) = Mass of steel * heat capacity of steel * ( Temperature final - temperature initial )
1600
E = mass x sp ht x Δ°tIn order to calculate the final temperature change, we must also find the temperature change.1. Find the temperature change.Divide joules by (mass x specific heat).Δ°t = 40,000J/500.0g x 4.184J/g°CΔ°t = 19.1°C2. Calculate the final temperature.Tf = 10.0 - 19.1Tf = -9.1°CThere was a decrease in temperature, indicating that it was an endothermic reaction (as energy was removed as stated in the question).
dude im not gonna do your homework for you.
54 degrees celcius