Thank you for visiting Calculate the energy required to convert 1 70 g of ice originally at 12 0 circ C into steam at 105 circ C. This page is designed to guide you through key points and clear explanations related to the topic at hand. We aim to make your learning experience smooth, insightful, and informative. Dive in and discover the answers you're looking for!
Answer :
Total energy: 6170.57 J. Steps: Heat ice, melt ice, heat water, vaporize water, heat steam.
To calculate the energy required to convert a substance through multiple phases, we need to consider the energy required for each phase transition and for heating or cooling within each phase.
Here are the steps to solve this problem:
1. Calculate the energy required to raise the temperature of the ice from -12.0°C to its melting point (0°C).
2. Calculate the energy required to melt the ice at 0°C.
3. Calculate the energy required to raise the temperature of the resulting water from 0°C to its boiling point (100°C).
4. Calculate the energy required to vaporize the water at 100°C.
5. Calculate the energy required to raise the temperature of the resulting steam from 100°C to 105°C.
Let's start with the calculations:
1. Energy to raise the temperature of ice:
[tex]\[ q_1 = m \cdot c_{\text{ice}} \cdot \Delta T \][/tex]
[tex]\[ q_1 = 1.70 \, \text{g} \times 2.09 \, \text{J/g\°C} \times (0 - (-12)) \, \text{\°C} \][/tex]
[tex]\[ q_1 = 1.70 \, \text{g} \times 2.09 \, \text{J/g\°C} \times 12 \, \text{\°C} \][/tex]
[tex]\[ q_1 = 1.70 \, \text{g} \times 2.09 \, \text{J/g\°C} \times 12 \, \text{\°C} \][/tex]
[tex]\[ q_1 = 42.588 \, \text{J} \][/tex]
2. Energy to melt the ice:
[tex]\[ q_2 = m \cdot \Delta H_{\text{fusion}} \][/tex]
[tex]\[ q_2 = 1.70 \, \text{g} \times 334 \, \text{J/g} \][/tex]
[tex]\[ q_2 = 567.8 \, \text{J} \][/tex]
3. Energy to raise the temperature of water:
[tex]\[ q_3 = m \cdot c_{\text{water}} \cdot \Delta T \][/tex]
[tex]\[ q_3 = 1.70 \, \text{g} \times 4.18 \, \text{J/g\°C} \times (100 - 0) \, \text{\°C} \][/tex]
[tex]\[ q_3 = 1.70 \, \text{g} \times 4.18 \, \text{J/g\°C} \times 100 \, \text{\°C} \][/tex]
\[ q_3 = 710.92 \, \text{J} \]
4. Energy to vaporize the water:
[tex]\[ q_4 = m \cdot \Delta H_{\text{vap}} \][/tex]
[tex]\[ q_4 = 1.70 \, \text{g} \times 2260 \, \text{J/g} \][/tex]
[tex]\[ q_4 = 3832 \, \text{J} \][/tex]
5. Energy to raise the temperature of steam:
[tex]\[ q_5 = m \cdot c_{\text{steam}} \cdot \Delta T \][/tex]
[tex]\[ q_5 = 1.70 \, \text{g} \times 2.03 \, \text{J/g\°C} \times (105 - 100) \, \text{\°C} \][/tex]
[tex]\[ q_5 = 1.70 \, \text{g} \times 2.03 \, \text{J/g\°C} \times 5 \, \text{\°C} \][/tex]
[tex]\[ q_5 = 17.255 \, \text{J} \][/tex]
Now, sum up all these energies to find the total energy required:
[tex]\[ \text{Total energy} = q_1 + q_2 + q_3 + q_4 + q_5 \][/tex]
[tex]\[ \text{Total energy} = 42.588 \, \text{J} + 567.8 \, \text{J} + 710.92 \, \text{J} + 3832 \, \text{J} + 17.255 \, \text{J} \][/tex]
[tex]\[ \text{Total energy} = 6170.565 \, \text{J} \][/tex]
So, the total energy required to convert 1.70 g of ice originally at –12.0°C into steam at 105°C is approximately [tex]\( 6170.57 \, \text{J} \).[/tex]
Thank you for reading the article Calculate the energy required to convert 1 70 g of ice originally at 12 0 circ C into steam at 105 circ C. We hope the information provided is useful and helps you understand this topic better. Feel free to explore more helpful content on our website!
- You are operating a recreational vessel less than 39 4 feet long on federally controlled waters Which of the following is a legal sound device
- Which step should a food worker complete to prevent cross contact when preparing and serving an allergen free meal A Clean and sanitize all surfaces
- For one month Siera calculated her hometown s average high temperature in degrees Fahrenheit She wants to convert that temperature from degrees Fahrenheit to degrees
Rewritten by : Jeany
