Question

The specific heat of silver (ag) is 0.245 j/ºc g. determine the energy required to raise the temperature of 350 g of ag from 293 k to 400 k.

Answer 1

Specific heat equation is given as

$Q =m\times c\times \Delta T$

where, Q = energy required

m = mass

c = specific heat

$\Delta T$ = change in temperature

Specific heat of silver ($Ag$) is $0.245 J/^{o}C g$

Mass of silver  = 350 g

$\Delta T =T_{final}-T_{intital}$

Convert 400 K to degree Celsius = 400-273 = 127 K

Convert 293 K to degree Celsius = 293-273 = 20 K

Thus, $\Delta T =127 K-20 K$

=   $107^{o}C$

Put the values,

$Q =m\times c\times \Delta T$

$Q = 350 g\times 0.245 J/^{o}C g\times(107^{o}C)$

= 9175.25 J

Hence, energy required to raise the temperature is 9175.25 J

Answer 2

9180 Joules First determine how many degrees the temperature is being changed. 400 K - 293 K = 107 K Since the units K and C have the same magnitude (they just have a different 0 point). We can freely exchange them when merely speaking of differences and not absolute values. So we can express the specific heat of silver as 0.245 J/ÂşC g or 0.245 J/K g. In any case, we now have 3 values with the units J/K g, g, and K. We desire a result with the units J. So it's a simple matter of multiplication and division such that we get the desired unit. Let's start with our specific heat 0.245 J/(K g) And let's cancel out the g term. Multiplying by our g term will do nicely. So 0.245 J/(K g) * 350 g = 85.75 J/K Now let's cancel out the K term. Another multiplication will do it. 85.75 J/K * 107 K = 9175.25 J Since we only have 3 significant figures in our data, round to 3 significant figures, giving 9180 J.