Welcome to Westonci.ca, your go-to destination for finding answers to all your questions. Join our expert community today! Get quick and reliable solutions to your questions from knowledgeable professionals on our comprehensive Q&A platform. Explore comprehensive solutions to your questions from knowledgeable professionals across various fields on our platform.
Sagot :
Sure! Let's walk through the problem step by step to find the heat change for the solution.
### Given Data:
1. Mass of the solution (m): \( 41.3 \, \text{g} \)
2. Specific heat capacity (c): \( 4.04 \, \text{J/g}^\circ\text{C} \)
3. Initial Temperature (T_initial): \( 21.2^\circ\text{C} \)
4. Final Temperature (T_final): \( 76.6^\circ\text{C} \)
### Formula for Heat Change:
The heat change for the solution can be calculated using the formula:
[tex]\[ q_{\text{soln}} = m \times c \times (T_f - T_i) \][/tex]
### Step-by-Step Solution:
1. Determine the temperature change (ΔT):
[tex]\[ ΔT = T_{\text{final}} - T_{\text{initial}} \][/tex]
[tex]\[ ΔT = 76.6^\circ\text{C} - 21.2^\circ\text{C} \][/tex]
[tex]\[ ΔT = 55.4^\circ\text{C} \][/tex]
2. Substitute the values into the formula:
[tex]\[ q_{\text{soln}} = 41.3 \, \text{g} \times 4.04 \, \text{J/g}^\circ\text{C} \times 55.4^\circ\text{C} \][/tex]
3. Calculate the heat change (q_soln):
[tex]\[ q_{\text{soln}} = 41.3 \times 4.04 \times 55.4 \][/tex]
4. The multiplication yields:
[tex]\[ q_{\text{soln}} = 9243.600799999998 \, \text{J} \][/tex]
### Final Result:
The heat change for the solution is [tex]\( 9243.600799999998 \, \text{J} \)[/tex].
### Given Data:
1. Mass of the solution (m): \( 41.3 \, \text{g} \)
2. Specific heat capacity (c): \( 4.04 \, \text{J/g}^\circ\text{C} \)
3. Initial Temperature (T_initial): \( 21.2^\circ\text{C} \)
4. Final Temperature (T_final): \( 76.6^\circ\text{C} \)
### Formula for Heat Change:
The heat change for the solution can be calculated using the formula:
[tex]\[ q_{\text{soln}} = m \times c \times (T_f - T_i) \][/tex]
### Step-by-Step Solution:
1. Determine the temperature change (ΔT):
[tex]\[ ΔT = T_{\text{final}} - T_{\text{initial}} \][/tex]
[tex]\[ ΔT = 76.6^\circ\text{C} - 21.2^\circ\text{C} \][/tex]
[tex]\[ ΔT = 55.4^\circ\text{C} \][/tex]
2. Substitute the values into the formula:
[tex]\[ q_{\text{soln}} = 41.3 \, \text{g} \times 4.04 \, \text{J/g}^\circ\text{C} \times 55.4^\circ\text{C} \][/tex]
3. Calculate the heat change (q_soln):
[tex]\[ q_{\text{soln}} = 41.3 \times 4.04 \times 55.4 \][/tex]
4. The multiplication yields:
[tex]\[ q_{\text{soln}} = 9243.600799999998 \, \text{J} \][/tex]
### Final Result:
The heat change for the solution is [tex]\( 9243.600799999998 \, \text{J} \)[/tex].
Thank you for trusting us with your questions. We're here to help you find accurate answers quickly and efficiently. Your visit means a lot to us. Don't hesitate to return for more reliable answers to any questions you may have. Thank you for trusting Westonci.ca. Don't forget to revisit us for more accurate and insightful answers.