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A 10.5 g block of iron metal (Cs= 0.449 J/g⁰C) at 55°C is submerged in 7.50...

A 10.5 g block of iron metal (Cs= 0.449 J/g⁰C) at 55°C is submerged in 7.50 mL water (Cs = 4.184 J/g⁰C) initially at 25°C (density of water is 1.00 g/mL). What is the final temperature of the iron and water?

-[(10.5 g)(0.449 J/(g℃))(Tf - 55℃)] = (7.50 g)(4.184J/(g℃))(Tf - 25℃)

Tf = 29 ℃

I understand how to set the problem up but do not understand how to isolate Tf by itself? Can someone show me the steps that were taken once the equation is set up? Thanks!

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