Asked by Cathy
Will someone show me the formula or help me through working this question? Thanks!
A 2.85g lead weight, initially at 10.3 deg C, is submerged in 7.55g of water at 52.3 deg C in an insulated container. what is the final temperature of both substances at thermal equilibrium?
A 2.85g lead weight, initially at 10.3 deg C, is submerged in 7.55g of water at 52.3 deg C in an insulated container. what is the final temperature of both substances at thermal equilibrium?
Answers
Answered by
bobpursley
formula? The concept is the closed container gains no heat from outside, so the sum of the heats gained is zero (one gains, one loses).
Heatgaindlead+heatgainedwater=0
2.85g*clead*(Tf-10.3C)+7.55g*cwater*(Tf-52.3)=0
look up the two specific heats (watch units, your mass is in grams). Solve for Tfinal.
Heatgaindlead+heatgainedwater=0
2.85g*clead*(Tf-10.3C)+7.55g*cwater*(Tf-52.3)=0
look up the two specific heats (watch units, your mass is in grams). Solve for Tfinal.
Answered by
Cathy
Alright thanks! Using what you gave me I got T= 53 degrees, hope that's right!
Answered by
bobpursley
I don't think so....the water was initially hotter, and putting cold lead in made it hotter? I don't think so. Recheck.
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