what is the formula for calculating heat?
280769
The equation for calculating heat energy is q=mCpΔT, where q is the heat variable, m is the mass of the object, Cp is the specific heat constant and ΔT is the temperature change.
447813
['P(kW) = √3 × PF × I(A) × VL-L(V) / 1000.', 'kilowatt = √3 × PF × amp × volt / 1000.', 'kW = √3 × PF × A × V / 1000.', 'P = √3 × 0.8 × 3A × 110V / 1000 = 0.457kW.']
1225239
['To figure the total kinetic energy, you multiply the average kinetic energy by the number of molecules you have, which is nNA, where n is the number of moles:', 'NAk equals R, the universal gas constant, so this equation becomes the following:']
1157365
The first law of thermodynamics is given as ΔU = Q − W, where ΔU is the change in internal energy of a system, Q is the net heat transfer (the sum of all heat transfer into and out of the system), and W is the net work done (the sum of all work done on or by the system).
1028278
The thermal energy is usually expressed by Q. It is directly proportional to the mass of the substance, temperature difference and the specific heat. The SI unit of thermal energy is Joules(J). ΔT = temperature difference.
148332
['Calculate the heat released, q, in joules (J), by the reaction: q = mass(water) × specific heat capacity(water) × change in temperature(solution) ... ', 'Calculate the moles of solute (NaOH(s)): moles = mass ÷ molar mass. ... ', 'Calculate the enthalpy change, ΔH, in kJ mol-1 of solute:']
57066
Since the temperature doesn't change (at least not usually) during a phase change we cannot use the formula q=mcΔT to calculate the heat involved in that phase change. ... If the phase change is between liquid and gas the formula looks like q=mΔ vap and ΔH vap is called the heat of vaporization.
419097
K = (QL)/(AΔT) K is the thermal conductivity in W/m.K. Q is the amount of heat transferred through the material in Joules/second or Watts. L is the distance between the two isothermal planes. A is the area of the surface in square meters.
1357396
The heat of an object is the total energy of all the molecular motion inside that object. Temperature is the measure of the thermal energy or average heat of the molecules in a substance. It's a measure of the number of atoms multiplied by the energy possessed by each atom.
1070075
Heat is a measure of change, never a property possessed by an object or system. Therefore, it is classified as a process variable. Temperature describes the average kinetic energy of molecules within a material or system and is measured in Celsius (°C), Kelvin(K), Fahrenheit (°F), or Rankine (R).
1235638
['Δ = A change in enthalpy.', "o = A degree signifies that it's a standard enthalpy change.", 'f = The f indicates that the substance is formed from its elements.']
607808
0 degrees Celsius is equal to 32 degrees Fahrenheit. The basic formula is (°C × 9/5) + 32 = °F. 0 degrees Celsius is equal to 273.15 Kelvins.
1313833
Q in the above equation is -ΔH and is expressed in kJ/mol of water. Neutralization reactions are generally exothermic and thus ΔH is negative. Heat measurements are performed by carrying out the reaction in a special container called a calorimeter.
244372
The general equation for an endothermic reaction is: Reactants + Energy → Products. In endothermic reactions, the temperature of the products is typically lower than the temperature of the reactants.
491849
Heat is the transfer of thermal energy from a system to its surroundings or from one object to another. This transfer of energy is from the object at a higher temperature to the object at a lower temperature.
34930
Calculate the kilowatt-hours (kWh) required to heat the water using the following formula: Pt = (4.2 × L × T ) ÷ 3600. Pt is the power used to heat the water, in kWh. L is the number of liters of water that is being heated and T is the difference in temperature from what you started with, listed in degrees Celsius.
11031
The standard enthalpy of reaction, ΔH⊖rxn Δ H r x n ⊖ , can be calculated by summing the standard enthalpies of formation of the reactants and subtracting the value from the sum of the standard enthalpies of formation of the products.