q(joules) = mass * specific heat * change in temperature ( 8 kg = 8000 grams )
q = (8000 grams H2O)(4.180 J/gC)(70o C - 20o C)
= 1.7 X 106 joules
============
1 joule = 2.39 X 10-4 kcal 65-30 = 35 degrees 1 kcal = 1 degree kg 35 degrees X 0.5 kg / 2.39 X 10-4 kcal/joulle = 73222 joules
E = mass x specific heat x Δ°T Δ°T = new temperature - original temperature where Δ°T is equal to temperature change (Celsius in this case). The specific heat of Al is 0.900 J/g°C. Before we proceed to find the quantity of heat in joules, we must first find the temperature change. To calculate the temperature change, we must subtract the original temperature from the new temperature. Δ°T = 50°C - 25°C = 25°C In order to find the quantity of heat (joules), we must multiply mass, specific heat, and the temperature change (calculated above). E = 40.0g x 0.900 J/g°C x 25°C = 900 Joules or 9.0 x 102 Joules
58 F
In order to walk from 15 below ground to 45 above ground, you have to climb a total of 60 floors.
You need the heat capacities for these substances in order to answer this question. If you have those, it's simple algebra.
1 joule = 2.39 X 10-4 kcal 65-30 = 35 degrees 1 kcal = 1 degree kg 35 degrees X 0.5 kg / 2.39 X 10-4 kcal/joulle = 73222 joules
E = mass x specific heat x Δ°T Δ°T = new temperature - original temperature where Δ°T is equal to temperature change (Celsius in this case). The specific heat of Al is 0.900 J/g°C. Before we proceed to find the quantity of heat in joules, we must first find the temperature change. To calculate the temperature change, we must subtract the original temperature from the new temperature. Δ°T = 50°C - 25°C = 25°C In order to find the quantity of heat (joules), we must multiply mass, specific heat, and the temperature change (calculated above). E = 40.0g x 0.900 J/g°C x 25°C = 900 Joules or 9.0 x 102 Joules
E = mass x specific heat x Δ°t (temperature change)------------------ Energyspecific heat * temperature change = massΔ°t = new temperature - original temperatureIn order to calculate the mass of water able to be heated, we must divide the given energy by the result of specific heat times temperature change. Before proceeding to do such, we must calculate the temperature change, as well as convert cal to joules. It is also important to know that water's specific heat is 4.184 J/g°C.1. Calculate temperature change.Δ°t = 100°C-25°CΔ°t= 75°C2. Convert kcal to joules (multiply kcal * 103 * 4.184 joules [J]). (kcal --> joules)Joules = 4.22 kcal x 103 cal x 4.184 J/g°C = 17656.48 Joules------------------------ 1 kcal ------ 1 cal3. Find mass.Mass = 17656.48J(4.184J/g°C * 75°C) = 56.3g
Fahrenheit is a temperature scale in which water freezes at 32 degrees and boils at 212 degrees
82 degrees C !!!
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).
In order for water to reach it's boiling point, then the temperature has to reach 212 degrees. 212 degrees is for about sea level. it will vary depending on where you are.
Clay needs to be heated to a temperature of around 1,000 to 1,300 degrees Fahrenheit in order to harden.
According to the NHL, the ice is supposed to remain between 20 and 22 degrees Fahrenheit; with 22 degrees being the optimal ice temperature. The temperature inside the arena itself is supposed to remain below 65 degrees.
The degrees go in order from coldest to hottest when measuring temperature. The scale typically starts at absolute zero, then goes up through negative numbers, zero, and then positive numbers.
To calculate the heat absorbed by the water, you can use the formula ( Q = mc\Delta T ), where ( Q ) is the heat absorbed, ( m ) is the mass of the water, ( c ) is the specific heat capacity of water (approximately 4.18 J/g°C), and ( \Delta T ) is the change in temperature. For a 500 g pot of water raising the temperature from 20°C to 30°C (( \Delta T = 10°C )), the calculation would be: [ Q = 500 , \text{g} \times 4.18 , \text{J/g°C} \times 10 , \text{°C} = 20,900 , \text{J} ] Thus, 20,900 joules of heat must be absorbed.
A freezer should be set to a temperature of 0 degrees Fahrenheit (-18 degrees Celsius) to properly preserve food.