2 part question
1 answer:
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Answer:
115 ⁰C
Explanation:
<u>Step 1:</u> The heat needed to melt the solid at its melting point will come from the warmer water sample. This implies
-----eqution 1
where,
is the heat absorbed by the solid at 0⁰C
is the heat absorbed by the liquid at 0⁰C
the heat lost by the warmer water sample
Important equations to be used in solving this problem
, where -----equation 2
q is heat absorbed/lost
m is mass of the sample
c is specific heat of water, = 4.18 J/0⁰C
is change in temperature
Again,
-------equation 3
where,
q is heat absorbed
n is the number of moles of water
tex]\delta {_f_u_s}[/tex] is the molar heat of fusion of water, = 6.01 kJ/mol
<u>Step 2:</u> calculate how many moles of water you have in the 100.0-g sample
<u>Step 3: </u>calculate how much heat is needed to allow the sample to go from solid at 218⁰C to liquid at 0⁰C
This means that equation (1) becomes
79.13 KJ +
<u>Step 4:</u> calculate the final temperature of the water
Substitute in the values; we will have,
79.13 kJ + 990.66J* = -1463J*
Convert the joules to kilo-joules to get
79.13 kJ + 0.99066KJ* = -1.463KJ*
collect like terms,
2.45366 = 283.133
∴ = 115.4 ⁰C
Approximately the final temperature of the mixture is 115 ⁰C