Let's go through this step-by-step.
1. Given Data:
- Mass of water ([tex]\( m \)[/tex]) = 50 grams
- Specific heat capacity of water ([tex]\( c \)[/tex]) = 4.186 J/g°C
- Temperature change ([tex]\( \Delta T \)[/tex]) = 5.53°C
2. Write the formula:
The amount of heat ([tex]\( Q \)[/tex]) required to change the temperature of a substance is given by the formula:
[tex]\[
Q = mc\Delta T
\][/tex]
3. Plug in the values:
Substitute the given values into the formula:
[tex]\[
Q = (50 \, \text{g}) \times (4.186 \, \text{J/g°C}) \times (5.53 \, \text{°C})
\][/tex]
4. Calculate [tex]\( Q \)[/tex]:
Calculate the product
[tex]\[
Q = 50 \times 4.186 \times 5.53
\][/tex]
After performing the multiplication, we get:
[tex]\[
Q = 1157.429 \, \text{J}
\][/tex]
5. Convert Joules to kilojoules:
1 kJ = 1000 J
[tex]\[
Q_{\text{kJ}} = \frac{1157.429 \, \text{J}}{1000} = 1.157429 \, \text{kJ}
\][/tex]
6. Round to the nearest 10 kJ:
Looking at the value 1.157429 kJ, when rounding to the nearest 10 kJ:
[tex]\[
\text{Rounded value} = 0 \, \text{kJ}
\][/tex]
Answer:
So, the amount of heat produced, rounded to the nearest 10 kJ, is:
[tex]\[ \text{0} \, \text{kJ} \][/tex]
