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The specific heat of water is 4.18J/gcdot ^circ C How much heat does 225.0 g of water release when it cools from 85.5^circ C to 50.0^circ C Use the formula q=mC,Delta T. 3.26times 10^4J 3.34times 10^4J 1.27times 10^5J 2.90times 10^5J

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The specific heat of water is 4.18J/gcdot ^circ C How much heat does 225.0 g of water release when it cools from 85.5^circ C to 50.0^circ C Use the formula q=mC,Delta T. 3.26times 10^4J 3.34times 10^4J 1.27times 10^5J 2.90times 10^5J

The specific heat of water is 4.18J/gcdot ^circ C How much heat does 225.0 g of water release when it cools from 85.5^circ C to 50.0^circ C Use the formula q=mC,Delta T. 3.26times 10^4J 3.34times 10^4J 1.27times 10^5J 2.90times 10^5J

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XavierProfessional · Tutor for 6 years

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Sure, let's work through the problem step by step.Question:How much heat does \(225.0 \, \text{g}\) of water release when it cools from \(85.5^{\circ} \, \text{C}\) to \(50.0^{\circ} \, \text{C}\)?Given formula: \(q = m \cdot C_{p} \cdot \Delta T\)Step 1:Identify the values given in the problem:- Mass (\(m\)): \(225.0 \, \text{g}\)- Specific heat of water (\(C_{p}\)): \(4.18 \, \text{J/g}^{\circ} \text{C}\)- Initial temperature (\(T_{\text{initial}}\)): \(85.5^{\circ} \, \text{C}\)- Final temperature (\(T_{\text{final}}\)): \(50.0^{\circ} \, \text{C}\)Step 2:Calculate the temperature change (\(\Delta T\)):\[\Delta T = T_{\text{final}} - T_{\text{initial}}\]\[\Delta T = 50.0^{\circ} \, \text{C} - 85.5^{\circ} \, \text{C}\]Step 3:Now, substitute the values into the formula:\[q = m \cdot C_{p} \cdot \Delta T\]Step 4:Calculate the heat (\(q\)):\[q = 225.0 \, \text{g} \cdot 4.18 \, \text{J/g}^{\circ} \text{C} \cdot (\Delta T)\]Step 5:Solve for \(\Delta T\) and substitute the values:\[q = 225.0 \, \text{g} \cdot 4.18 \, \text{J/g}^{\circ} \text{C} \cdot (50.0^{\circ} \, \text{C} - 85.5^{\circ} \, \text{C})\]Now, calculate the value of \(q\).Step 6:Take a deep breath and perform the calculation to get the final answer.\[q \approx 3.26 \times 10^{4} \, \text{J}\]So, the correct answer is \(3.26 \times 10^{4} \, \text{J}\).**Answer:**\[3.26 \times 10^{4} \, \text{J}\]DONE
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