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dangina
2 months ago
15

A 2.40 kg block of ice is heated with 5820 J of heat. The specific heat of water is 4.18 J•g^-1•C^-1. By how much will it’s temp

erature rise, assuming it does not melt?
Chemistry
1 answer:
lorasvet [2.7K]2 months ago
0 0

Response: The increase in temperature is 0.53^0C

Reasoning:

The amount of thermal energy needed to elevate the temperature of a given substance by one degree Celsius is referred to as the specific heat capacity.

Q=m\times c\times \Delta T

Q = Heat gained by ice = 5280 J

m = mass of ice = 2.40 kg = 2400 g   (1kg=1000g)

c = heat capacity of water = 4.18J/g^0C

Initial temperature  = T_i

Final temperature = T_f  

Temperature change ,\Delta T=T_f-T_i=?

Substituting the values, we obtain:

5280J=2400g\times 4.18J/g^0C\times \Delta T

\Delta T=0.53^0C

Therefore, the temperature increase is 0.53^0C

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A white powder is known to be a mixture of magnesium oxide and aluminum oxide. 100cm3 of 2moldm-3 NaOH(aq) is just sufficient to
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An experimenter studying the oxidation of fatty acids in extracts of liver found that when palmitate (16:0) was provided as subs
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The conversion of CO2 and propionyl-CoA into methylmalonyl-CoA is catalyzed by propionyl-CoA carboxylase, which contains biotin. The function of biotin is to activate CO₂ before it is transferred to the propionate group. The addition of avidin obstructs the complete oxidation of undecanoic acid as it binds very tightly to biotin, thereby hindering the activation and transfer of CO₂ to propionate.

In contrast, palmitate oxidation does not require carboxylation, meaning that the presence of avidin doesn't influence its oxidation.

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