4.05 kg + 567.95 g + 100.1 g add the correct value using the correct sig figs and or least precise degree of precision. When i d
1 answer:
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Clarification:
The pertinent information is outlined as follows.
m = 10.0 kg = 10,000 g (since 1 kg = 1000 g)
Starting temperature of block 1, = (100 + 273) K = 373 K
Starting temperature of block 2, = (0 + 273) K = 273 K
Therefore, the heat lost by block 1 equals the heat received by block 2
It's important to convert the temperature into Kelvin as (50 + 273) K = 323 K.
Additionally, the relationship between enthalpy and temperature change is as follows.
=
= 1243550 J
or, = 1243.5 kJ
Next, determine the entropy change for block 1 as follows.
=
=
= -554.12 J/K
Now, the entropy change for block 2 is as follows.
=
=
= 647.49 J/K
Thus, the total entropy is the sum of the entropy changes of both blocks.
= -554.12 J/K + 647.49 J/K
= 93.37 J/K
In conclusion, for this reaction, the outcome is 1243.5 kJ and is 93.37 J/K.