Wiki User
∙ 15y agoIt takes 4.186 Joules to heat one gram of water by 1-degree Celsius.
4.186 * 4000 = 16,744 Joules to heat 4 kilos of water by 1-degree.
16,744 * 70 = 1,172,080 Joules.
The above assumes that one litre of water weighs exactly 1 Kilogram.
Wiki User
∙ 15y agoThe specific heat capacity of water is 4.18 J/g°C. The mass of water is 4000 g. The temperature change is 70.0°C - 0°C = 70.0°C. Therefore, the heat required is 4.18 J/g°C x 4000 g x 70.0°C = 1,170,400 J.
Wiki User
∙ 12y agoConversion needed.
4 kg (1000 grams/1 kg)
= 4000 grams
----------------------now,
q(thermal energy in Joules) = mass * specific heat * change in temperature
q = (4000 grams)(4.180 J/gC)(75 C - 25 C)
= 8.4 X 105 Joules
--------------------------
Approx 2940 Joules.
To convert 50 kg of water at 80 degrees Celsius to steam at 100 degrees Celsius, you need to calculate the heat energy needed to raise the temperature of water from 80 to 100 degrees Celsius (specific heat capacity of water) and then the heat energy needed for water to steam phase change (latent heat of vaporization of water). The total heat energy required can be calculated using the formula: Q = mcΔT + mL, where Q is the heat energy, m is the mass, c is the specific heat capacity, ΔT is the temperature change, and L is the latent heat of vaporization.
The specific heat capacity of water is 4.18 J/g°C, which means it takes 4.18 Joules of energy to raise 1 gram of water by 1 degree Celsius. To raise the temperature of 8.1 g of water by 20 degrees Celsius, you would need 8.1 g * 20°C * 4.18 J/g°C = 676.56 Joules of energy.
The amount of energy needed to reduce water temperature from 15 degrees to 14 degrees depends on the mass of the water and its specific heat capacity. Typically, it would require a minimal amount of energy to achieve such a small temperature change in a small quantity of water.
Approx. 600 - 800 degrees C / 1,100 - 1,500 degrees F
8.200 J
The specific heat capacity of water is 4.18 Joules/gram degrees Celsius. Therefore, it would take 4.18 Joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.
It takes 4.184 joules of energy to change the temperature of 1 gram of water by 1 degree Celsius.
Approx 2940 Joules.
I will use this formula. Some conversion will be required. ( I only know specific heat iron in J/gC ) q(Joules) = mass * specific heat * change in temperature Celsius 3 kilograms cast iron = 3000 grams q = (3000 g)(0.46 J/gC)(120 C - 30 C) = 124200 Joules (1 kilojoule/1000 joules) = 124.2 kilojoules of energy needed ===========================
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
The specific heat capacity of water is 4.186 J/g°C. Since there are 1000 grams in a kilogram, it would require 20,930 Joules of energy to increase the temperature of a kilogram of water by 5 degrees Celsius.
The specific heat of air at 0 degrees Celsius is 1.01 Joules per gram or J/g. The specific heat of a substance is defined as the quantity of heat per unit mass needed to raise its temperature by one degree Celsius.
The amount of heat needed to raise the temperature of 1 kilogram of water by 1 degree Celsius is 4186 Joules, which is the specific heat capacity of water.
A fever. Normal body temperature is around 37 degrees Celsius, so 40 degrees Celsius would indicate a fever. It would be a good idea to monitor your symptoms and consult with a healthcare provider if needed.
The relevant equation behind this problem is Q=m*c* ΔT Where Q is the energy that must be added to or taken from the system, m is the mass of the object, c is the objects specific heat, and ΔT is the change in temperature in Celsius or Kelvin. Plugging in the given values we get that Q=.015kg * 128J/(kg*C) * 10C=19.2J. Therefore, you need 19.2 joules of heat in order to raise the temperature of a .015kg sample of lead by 10 degrees Celsius.
To convert 50 kg of water at 80 degrees Celsius to steam at 100 degrees Celsius, you need to calculate the heat energy needed to raise the temperature of water from 80 to 100 degrees Celsius (specific heat capacity of water) and then the heat energy needed for water to steam phase change (latent heat of vaporization of water). The total heat energy required can be calculated using the formula: Q = mcΔT + mL, where Q is the heat energy, m is the mass, c is the specific heat capacity, ΔT is the temperature change, and L is the latent heat of vaporization.