HEAT Q=c*m(t2-t1) c=0.24 (specific heat of sand) t2-t1=100.0oc-20.0oc=80.0oc m=1.40kgQ=0.24*1.40*80.0 Q=26.88 kilocalories or Q=26880 calories
q= m Cs (change in temperature)
change in temperature = final temperature - initial temperature ==> 100.0 C- 30.0 C =70C
specific heat capacity of sand (Cs) = .84 J/ g * deg C
mass = 1.7kg ==> convert to grams ==> 1700g
just plug those in to find q which is the amount of heat
q = (1700g) (.84 g/ J *deg C) (70.0 C)
the units should cancel out to give you ....
q =99960 J ==> 100000J (for 3 sig fig if needed)
The heat required, Q , is given by:
Q = ( m ) ( Csh ) ( T2 - T1 )
Q = ( 1.60 kg ) ( 800 J/kg - C ) ( 100.0 C - 22.0 C )
Q = 99800 J <-------
The specific heat of sand, Csh , is a typical value from Heat Transfer Textbook. The
properties of sand can vary considerably, since sand varies a great deal in its composition, moisture content, etc.
It is going to take about 110 kJ to do this heating up. The formula that you will need to use is Q=m*Cp*dT.
b
how much heat is required to convert 0,3kg of ice at 0c to water at the same tempture
Heat required = mass x specific heat of water x temperature difference Here we have heat required = 21 x 1 x 10 = 210 cals
it depends how cold the ice is
The molar heat of fusion of water in J / g is 334. To find the heat required to convert 0.3 kg, use the equation: heat of fusion * mass = heat required. It would require 100.2 kJ.
b
heat of fusion
How much heat (in calories) is required to heat a 43 g sample of aluminum from 72 F to 145F
how much heat is required to convert 0,3kg of ice at 0c to water at the same tempture
How much heat energy is required to raise the temperature of 0.358 of copper from 23.0 to 60.0 ? The specific heat of copper is 0.0920
125.6kj (apex)
lf = 3.35 x 105 J kg-1 This much amount of heat required to convert 1 kg of ice to liquid Mani.Ra
Heat required = mass x specific heat of water x temperature difference Here we have heat required = 21 x 1 x 10 = 210 cals
The values are different for each type of plastic.
it depends how cold the ice is
No heat (energy) is required to freeze water (from liquid to solid). Freezing RELEASES energy (heat), as it is an exothermic event. If you want to know how much energy is release, you need to know the heat of fusion for water, and then multiply that by the mass of water being frozen.
The molar heat of fusion of water in J / g is 334. To find the heat required to convert 0.3 kg, use the equation: heat of fusion * mass = heat required. It would require 100.2 kJ.