Chemistry, 16.06.2020 01:57 karenpazyuli

A 81.1 g of ice, initially at - 22.30 C , is dropped in into 324.2 g of water at 87.80 C in an insulated container. What is the final temperature of the water when thermal equilibrium isreached?

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Answer from: linkaye3031

The final temperature of the water when thermal equilibrium is reached is 52.061 °C.

Explanation:

According to the First Law of Thermodynamics, which is a generalization of the Principle of Energy Conservation, energy cannot be created nor destroyed. In this case, ice enters in hot water and hot water releases heat until both elements reach thermal equilibrium. The consideration of an isolated system means the inexistence of any mass and energy interactions between system and surroundings.

Empirically speaking, ice is melt and reaches thermal equilibrium with rest of water. The system experiments the following changes:

1) Ice is melt and turns into water before reaching thermal equilibrium. (Positive change in internal energy)

2) Hot water is cooled before reaching thermal equilibrium. (Negative change in internal energy)

$\Delta U_{ice} + \Delta U_{hot\,water} = 0$

Change in internal energy in solids and liquids is equal to:

$\Delta U = m\cdot c\cdot \Delta T$

Where:

- Mass of the sample, measured in kilograms.

- Specific heat, measured in $\frac{kJ}{kg\cdot ^{\circ}C}$ .

$\Delta T$ - Change in temperature, measured in $^{\circ}C$ .

Besides, change in internal energy associated with phase changes is equal to:

$\Delta U = m \cdot L_{f}$

Where $L_{f}$ is the latent heat of fussion, measured in $\frac{kJ}{kg}$ .

Then, previous energy equation is expanded as follows:

$m_{ice}\cdot (c_{ice}\cdot \Delta T_{1} + L_{f, ice} + c_{water} \cdot \Delta T_{2}) + m_{hot\,water}\cdot c_{water}\cdot \Delta T_{3} = 0$

Inputs are described below:

$m_{ice} = 0.081\,kg$ , $m_{hot\,water} = 0.324\,kg$ , $c_{ice} = 2.093\,\frac{kJ}{kg\cdot ^{\circ}C}$ , $c_{water} = 4.186\,\frac{kJ}{kg\cdot ^{\circ}C}$ , $L_{f,ice} = 334\,\frac{kJ}{kg}$

Temperature changes are:

$\Delta T_{1} = 0\,^{\circ}C - (-22.30\,^{\circ}C)$

$\Delta T_{1} = 22.30\,^{\circ}C$

$\Delta T_{2} = T - 0\,^{\circ}C$

$\Delta T_{2} = T$

$\Delta T_{3} = T - 87.80\,^{\circ}C$

After replacing known variables and simplifying resulting expression, the following expression is found:

$3.781\,kJ + 27.054\,kJ + 0.339\cdot T + 1.356\cdot T - 119.080\,kJ = 0$

$1.695\cdot T = 88.245\,kW$

Finally, the final temperature of the water when thermal temperature is reached is:

$T = 52.061\,^{\circ}C$

Answer from: Quest

explanation:

venn diagram is pictorial representation with of circles showing the relation between two finite sets or things. the intersection part of two circles conveys the relation present in between those sets or things.

here in the venn diagram of sand and salt two circles represent sand and salt. but the area falling under the intersection of these circle represents the mixture of sand and salt.

so, in a venn diagram the mixture will be placed in a middle that is in between the intersection of two circles.

Answer from: Quest

Abbreviated as mg-25.

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