3. suppose that during the icy hot lab that 65 kj of energy were transferred to 450 g of water at 20°c. what…

3. suppose that during the icy hot lab that 65 kj of energy were transferred to 450 g of water at 20°c. what would have been the final temperature of the water?

3. suppose that during the icy hot lab that 65 kj of energy were transferred to 450 g of water at 20°c. what would have been the final temperature of the water?

Answer

Explanation:

Step1: Convert units

Convert (Q = 65\space kJ) to (J): (Q=65\times10^{3}\space J), (m = 450\space g), (c = 4.18\space J/(g\cdot^{\circ}C)), (T_{i}=20^{\circ}C). Use the formula (Q = mc\Delta T=mc(T_{f}-T_{i})).

Step2: Solve for (T_{f})

Rearrange the formula for (T_{f}): (T_{f}=\frac{Q}{mc}+T_{i}). Substitute the values: (T_{f}=\frac{65\times 10^{3}}{450\times4.18}+20). First, calculate (\frac{65\times 10^{3}}{450\times4.18}=\frac{65000}{1881}\approx 34.56). Then (T_{f}=34.56 + 20).

Answer:

(54.56^{\circ}C)