Problem: If 50.0 mL of ethanol (density = 0.789 g/ mL) initially at 7.0 °C is mixed with 50.0 mL of water (density = 1.0 g/ mL) initially at 28.4 °C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?

FREE Expert Solution

- qwater = qethanol-(mcT)water =(mcT)ethanol


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Problem Details

If 50.0 mL of ethanol (density = 0.789 g/ mL) initially at 7.0 °C is mixed with 50.0 mL of water (density = 1.0 g/ mL) initially at 28.4 °C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Thermal Equilibrium concept. You can view video lessons to learn Thermal Equilibrium Or if you need more Thermal Equilibrium practice, you can also practice Thermal Equilibrium practice problems .

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Based on our data, we think this problem is relevant for Professor Wilson's class at CSU CHICO.