1) A piece of Fe metal with a mass of 0.350 kg at a temperature of 300 oC is add
ID: 1085596 • Letter: 1
Question
1) A piece of Fe metal with a mass of 0.350 kg at a temperature of 300 oC is added to 1.00 kg of H2O(l) at a temperature of 20 oC. What is the final equilibrium temperature of the H2O(l) and the Fe? The specific heat of the Fe metal is 0.502 J/g.oC and the specific heat of H2O is 4.18 J/g.oC.2)When 100.0 mL of CsOH are mixed with 50.0 mL of 0.400 M HCl in a coffee cup calorimeter, the following reaction occurs: CsOH(aq) + HCl(aq) = CsCl(aq) + H2O(l) The temperature of both solutions before mixing was 22.50 oC and rises to 24.28 oC. after the neutralization reaction. What is the enthalpy change for the reaction per mole of HCl? The densities of all solutions are 1.00 g/mL and the specific heat capacities of all solutions are 4.18 J/g.oC. 1) A piece of Fe metal with a mass of 0.350 kg at a temperature of 300 oC is added to 1.00 kg of H2O(l) at a temperature of 20 oC. What is the final equilibrium temperature of the H2O(l) and the Fe? The specific heat of the Fe metal is 0.502 J/g.oC and the specific heat of H2O is 4.18 J/g.oC.
2)When 100.0 mL of CsOH are mixed with 50.0 mL of 0.400 M HCl in a coffee cup calorimeter, the following reaction occurs: CsOH(aq) + HCl(aq) = CsCl(aq) + H2O(l) The temperature of both solutions before mixing was 22.50 oC and rises to 24.28 oC. after the neutralization reaction. What is the enthalpy change for the reaction per mole of HCl? The densities of all solutions are 1.00 g/mL and the specific heat capacities of all solutions are 4.18 J/g.oC. 1) A piece of Fe metal with a mass of 0.350 kg at a temperature of 300 oC is added to 1.00 kg of H2O(l) at a temperature of 20 oC. What is the final equilibrium temperature of the H2O(l) and the Fe? The specific heat of the Fe metal is 0.502 J/g.oC and the specific heat of H2O is 4.18 J/g.oC.
2)When 100.0 mL of CsOH are mixed with 50.0 mL of 0.400 M HCl in a coffee cup calorimeter, the following reaction occurs: CsOH(aq) + HCl(aq) = CsCl(aq) + H2O(l) The temperature of both solutions before mixing was 22.50 oC and rises to 24.28 oC. after the neutralization reaction. What is the enthalpy change for the reaction per mole of HCl? The densities of all solutions are 1.00 g/mL and the specific heat capacities of all solutions are 4.18 J/g.oC.
Explanation / Answer
Answer (1)
Heat lost by Fe Metal =Heat gained by water
mf*cf*Delta T=mw*cw*Delta T
350*0.502*(300-T)= 1000*4.18*(T-25)
52710-175.7T=4180T-104500
4355.7T=157210
T=36.09 degree C
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