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3 years ago

I will mark brainly , please help !

Chemistry

1 answer:

topjm [15]3 years ago

7 0

...a metal atom will *lose* electrons to form a *positive* cation and a nonmetal atom will *accept* electrons to form an *negative* anion.

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What quantity of energy, in joules, is required to raise the temperature of 425 g of tin from room temperature, 25.0 °C, to its

Rama09 [41]

Answer:

Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is 45.249 kiloJoules.

Explanation:

Mass of the tin ,m= 425 g

Heat capacity of the tin ,c= 0.227 J/g K

Initial temperature of the tin , $T_1$ = 25.0 °C = 298.15 K

Final temperature of the tin, $T_2$ = 231.9 °C = 505.05 K

Let the heat required to change the temperature of tin from 298.15 K to 505.05 K be Q.

$Q=mc\times (T_2-T_1)$

$=425 g\times 0.227 J/g K\times (505.05K - 298.15 K)=19,960.68 J=19.961 kJ$

Heat required to melt tin at 505.05 K be Q'

The heat of fusion of tin metal = $\Delta H_{fus}=59.2 J/g$

$Q'= m\times \Delta H_{fus}=425 g\times 59.2 J/g=25,287.5 J=25.288 kJ$

Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is:

= Q+Q' = 19.961 kJ + 25.288 kJ = 45.249 kJ

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