If the specific heat of methanol is 2.51 j/k-g, how many joules are required to raise the temperature of 50 g of methanol from 20oc to 70oc?
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Heat = mass CH3OH x spht CH3OH x delta T
= (50 g)(2.51 J/g K)(40 K) = 5020 J
Note that delta T is the same for K as for C.
Answer: The amount of heat required is 6275 J
Explanation:
To calculate the change in temperature, we use the equation:
\(q=mc\Delta T\)
where,
q = heat absorbed = ?
m = mass of methanol = 50 g
c = specific heat capacity of methanol = 2.51 J/g.K
\(\Delta T=\) = change in temperature = \(T_2-T_1=(70-20)^oC=50^oC=50K\) (change remains the same)
Putting values in above equation, we get:
\(q=50g\times 2.51J/g.K\times 50K\\\\q=6275J\)
Hence, the amount of heat required is 6275 J