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The specific heat of silver is 0.24 mc015-1jpg How many joules of energy are needed to warm 4.37 g of silver from 25.0mc015-2jpgC to 27.5mc015-3jpgC?
Wiki User
∙ 11y ago
Specific Heat
q = m x C x (Tf - Ti)
q = amount of heat energy gained or lost by substance = 1072 J
m = mass of sample in grams = 4.91g
C = heat capacity (J/g•oC) = 0.240 J/g•oC
Tf = final temperature = ? (melting point of silver)
Ti = initial temperature = 25oC
To solve for Tf:
q/m•C = Tf - Ti
Ti + q/m•C = Tf
25oC + 1072 J/(4.91g x 0.250 J/g•oC) = Tf
9.0 x 102 oC = Tf
(898oC rounded to two significant figures due to 25oC.)
Wiki User
∙ 9y ago
Wiki User
∙ 11y agoq=mcdeltaT
q=(4.37)(0.24g)(25.0 degrees C-27.5 degrees C)
= -2.62 J
Wiki User
∙ 12y agoq(Joules) = mass * specific heat * change in temp.
q = (4.37 g)(0.237 J/gC)(27.5o C - 25.0o C)
= 2.59 Joules
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Wiki User
∙ 6y agoThe necessary heat is: Q = 400 x 45 x 0,233 = 4,194 kJ
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