you mixed 49.82g of NaCl ([NaCl]=3.395±0.05%) with 49.87g of NaOH ([NaOH]=3.761±0.05%) in a coffee cup calorimeter,...
you mixed 49.82g of NaCl ([NaCl]=3.395±0.05%) with 49.87g of NaOH ([NaOH]=3.761±0.05%) in a coffee cup calorimeter, The initial temperature is 22.62˚C, the final temperature is 29.30˚C.
1)What is the limiting reagent?
2)What total enthalpy of neutralization was released by the reaction (given that ∆H˚=-56.02 kJ/mol)?
3)What is the heat capacity of the calorimeter system(Cp, cal)?
Homework Answers
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you mixed 49.82g of NaCl ([NaCl]=3.395±0.05%) with 49.87g of
NaOH ([NaOH]=3.761±0.05%) in a coffee cup calorimeter,...
In a coffee cup calorimeter, 100.0 mL of 1.00 M NaOH and 200.0 mL of 0.80...
In a coffee cup calorimeter, 100.0 mL of 1.00 M NaOH and 200.0 mL of 0.80 M HCl are mixed at 25.0oC. After the reaction, the temperature is 29.5 oC. Assuming all solutions have a density of 1.00 g/cm3 and a specific heat capacity of 4.18 J/oC g, what is the enthalpy change (kJ) for the balanced reaction? HCl(aq) + NaOH(aq) => NaCl(aq) + H2O(l)
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Question 19 5 pts In a coffee cup calorimeter, 6.70 g of NH.NO, is mixed with...
Question 19 5 pts In a coffee cup calorimeter, 6.70 g of NH.NO, is mixed with 75.0 g of water at an initial temperature of 25.0 °C. At the end of the dissolution, the final temperature of the mixture is 13.1 °C. With the assumption that the solution has the same specific heat capacity as water and is accompanied by no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH.NO, in kJ/mol. C 47.2 80.1...
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In a coffee cup calorimeter, 6.70 g of NH4NO3 is mixed with 75.0 g of water at an initial temperature of 25.0 °C. At the end of the dissolution, the final temperature of the mixture is 13.1 °C. With the assumption that the solution has the same specific heat capacity as water and is accompanied by no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in kJ/mol. en ott 46.6 94.5 47.2 3.0 80.1
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