how to calculate how much heat is released?
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:']
314793
A heating curve has been plotted for a solid object as shown in the figure. If the mass of the object is 200 g, then latent heat of vaporization for the material of the object, is [power supplied to the object is constant and equal to 1 kW] A .
613286
['Surface area: 42 square metres. Divided by.', 'Spreading rate: 11 square metres per litre. Multiplied by.', 'Number of coats: 2 coats. Equals.', '42/11 x 2 = 7.6 litres.']
117121
1 Answer. Heating 1.30 Kg of sand 70 degrees Celsius takes 80,000 Joules of heat.
978530
['kW/ton = 12 / EER.', 'kW/ton = 12 / (COP x 3.412)', 'COP = EER / 3.412.', 'COP = 12 / (kW/ton) / 3.412.', 'EER = 12 / (kW/ton)', 'EER = COP x 3.412.']
973554
Always calculate the change in temperature by subtracting the initial temperature from the final temperature, Tf - Ti . If the heat is transferred into the substance, the thermal energy of the substance will go up and so q will be positive.
946443
It is measured on the scales of Celsius, Fahrenheit and Kelvin. The temperature change depends on the amount of heat released or absorbed. Temperature difference = amount of heat absorbed or released/ mass of the body* specific heat of the body. ΔT = Q/m*c.
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.
884962
Every chemical reaction involves a change in free energy, called delta G (∆G). To calculate ∆G, subtract the amount of energy lost to entropy (∆S) from the total energy change of the system; this total energy change in the system is called enthalpy (∆H ): ΔG=ΔH−TΔS.
1222757
To find the vapor pressure at a given temperature, use the Clausius-Clapeyron equation: ln(P1/P2) = (ΔHvap/R)((1/T2) - (1/T1)). You could also use Raoult's Law to find the vapor pressure: Psolution=PsolventXsolvent.
708876
['Energy can be transferred between stores during motion. ... ', 'kinetic energy = 0.5 × mass × speed 2', 'This is when:', 'Calculate the initial kinetic store of the car in the previous example, if its mass is 1500 kg. ... ', 'So the value of the kinetic store is 12,000 J or 12 kJ.']
766694
['2H2 + O2 -> 2H2O. This means that for every 2 molecules of Hydrogen gas, one molecule of Oxygen is needed to make 2 molecules of water. ... ', 'Enthalpy of reaction = (Enthalpy of products) - (Enthalpy of reactants) ... ', 'Enthalpy= -285.83-(0+0)', 'This means Enthalpy of formation of water=-285.83kJ/mol.']
275037
The total amount of heat (qtotal) can be calculated by adding q1, q2, and q3: The answer is C. 87.7 kJ.
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).
1415891
Q = m*s*dT, where Q = heat, m = mass, s = specific heat, and dT is the change in temperature (T2 - T1). You can use this formula to calculate the specific heat.
456124
Add the change in temperature to your substance's original temperature to find its final heat. For example, if your water was initially at 24 degrees Celsius, its final temperature would be: 24 + 6, or 30 degrees Celsius.
37768
Use the formula ∆H = m x s x ∆T to solve. Once you have m, the mass of your reactants, s, the specific heat of your product, and ∆T, the temperature change from your reaction, you are prepared to find the enthalpy of reaction. Simply plug your values into the formula ∆H = m x s x ∆T and multiply to solve.