Asked by Bob
How much heat, in kilojoules (kJ), is required to raise the temperature of 2.50kg Hg(l) from -20.0 to -6.0C? Assume a density of 13.6g/ml and a molar heat capacity of 28.0 J mol -1 C -1 for Hg(l).
Please helpppppp .... thanks in advance
Please helpppppp .... thanks in advance
Answers
Answered by
Jai
Through out the temperature range, Hg remains as liquid.
Recall that heat released or absorbed is given by
Q = m*c*(T2 - T1)
where
m = mass
c = specific heat
T = temperature
Note that molar mass of Hg is 200.6 g/mol.
Substituting,
Q = (250000 / 200.6)*(28.0)*(-6 -(-20))
Q = ?
Now solve for Q. The units are in J, so divide by 1000 to convert to kJ.
Hope this helps :3
Recall that heat released or absorbed is given by
Q = m*c*(T2 - T1)
where
m = mass
c = specific heat
T = temperature
Note that molar mass of Hg is 200.6 g/mol.
Substituting,
Q = (250000 / 200.6)*(28.0)*(-6 -(-20))
Q = ?
Now solve for Q. The units are in J, so divide by 1000 to convert to kJ.
Hope this helps :3
Answered by
Jai
*sorry, my conversion of 2.5 kg to g is wrong. The equation should be
Q = (2500 / 200.6)*(28.0)*(-6 -(-20))
Q = (2500 / 200.6)*(28.0)*(-6 -(-20))
Answered by
Anonymous
How much heat is required to raise the temperature of a 2.0 kg of water (specific heat = 1.0 cal/g°C) from 5.0°C to 100.0°C?
Answered by
Aasma
Why the density of Hg is given here in above question
-from Pakistan
-from Pakistan