a 15.7g aluminum block is wequipped to 53.2 C and plunged right into an insulated beaker containing 32.5g of water initially at 24.5 C. The aluminum and water are permitted to pertained to thermal equilibrium. Assuming that no warm is lost, what is the final temperature of the water and also aluminum.

You are watching: Assuming that no heat is lost, what is the final temperature of the water and aluminum?

I don't know what to do right here. Typically I simply plug in numbers to the warmth equation to acquire a final number of the joules necessary to reach a particular temperature and so on.

With this information I plugged it right into 2 different warmth equations:

aluminum: q = 15.7g * .903j/g celsius * (53.2 celsius - T)

water: q = 32.5g * 4.184j/g celsius * (Tlast - 24.5 celsius)

I'm trying to find the last temperature of both of them unified. What perform I do next?


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level 1
· 3y
The warm lost by the aluminum is equal to the heat gained by the water. Do an appropriate substitution.


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level 2
· 3y

How do I discover the warmth (q) in the aluminum component. I carry out not understand the starting temperature of the block of aluminum.

So I assume I would uncover q, and also plug q into the water one below, and also deal with for the final temp.

See more: A Comparison Of Two Amounts Using Division ? Topic 18: Compare And Order Rational Numbers


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level 1
· 3y
Qal = Q water and also find the last temperature! lower than 53.2 and also greater than 24.5! hope that helps


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