So I'm working on a free-standing question in TBR GChem :
"If a 20.0g piece of metal at 75 C with a heat capacity of 0.50 cal/g*K were added to 40g H20 at 25 C, then what would the equilibrium temperature be, assuming no loss of heat to the environment?"
I know how to set up the problem using MCdeltaT water = MCdeltaT metal
so, (40)(1.00)(Tf - 25)K = (20)(0.50)(Tf-75)K
= 40(Tf - 25) = 10(Tf - 75)
= 40Tf - 1000 = 10Tf - 750
= 30Tf = 250
Tf = 8.3 degrees Celcius ... but that's not...
Help me with my math?
"If a 20.0g piece of metal at 75 C with a heat capacity of 0.50 cal/g*K were added to 40g H20 at 25 C, then what would the equilibrium temperature be, assuming no loss of heat to the environment?"
I know how to set up the problem using MCdeltaT water = MCdeltaT metal
so, (40)(1.00)(Tf - 25)K = (20)(0.50)(Tf-75)K
= 40(Tf - 25) = 10(Tf - 75)
= 40Tf - 1000 = 10Tf - 750
= 30Tf = 250
Tf = 8.3 degrees Celcius ... but that's not...
Help me with my math?