When 1.10 g of a salt dissolves in 252 mL of water (density = 1.00 g/mL) in a coffee-cup calorimeter, the temperature rises from 16.1°C to 24.5°C. Determine q for the solution process, assuming that Ccal ≈ Cwater.
When 1.10 g of a salt dissolves in 252 mL of water (density = 1.00 g/mL)...
When 1.00 g of CaCl2 is added to 50.0 g of water in a coffee-cup calorimeter, it dissolves according to the following eqn: CaCl2 (s) Ca2 (aq) + 2Cl (aq) The temperature of the solution rises from 25.00°C to 28.51 °C. Assuming that all the heat flow involved in the reaction is transferred to the water, calculate q Also, assume that the csoln is equal to cwater Which is 4.18 J/g °C
find enthalpy change 3. When 2.617 g of AX (s) dissolves in 141.2 g of water in a coffee-cup calorimeter the temperature rises from 24.5 °C to 36.5 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX(s) - A+ (aq) + X(aq) Assumptions for this calculation: The specific heat of the solution is the same as that of pure water (4.18 J/gK) The density of water = 1.000 g/mL. The liquid's final volume is not changed by...
When a 9.55 g sample of solid NaOH dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 23.6C to 47 for the solution process. (Assume that the specific heat of the solution is the same as that of pure water.) . .4 °C. Calculate AH (in kJ/mol NaOH)
1. 5.00 g of urea, (NH2)2CO is dissolved in 250.0 mL of water(density = 1.00 g/mL) at 30.0oC in a coffee cup calorimeter. When this is done, 27.6 kJ of heat is absorbed. (5 points) a) Is the solution process exothermic or endothermic? c) What is qwater? d) What is the final temperature of the solution(specific heat constant of water is 4.18 J/g.OC)? Please show all the work!! thank you very much :)
5.55 When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 21.6 °C to 37.8 °C. Calculate ?? (in kJ/mol NaOH) for the solution process NaOH(s)-Na"(aq) + OH-(aq) Assume that the specific heat of the solution is the same as that of pure water.
When 10.00 mL of a solution of strong acid is mixed with 100.00 mL of a solution of weak base in a coffee-cup calorimeter, the temperature rises from 22.6 oC to 27.6 oC. Determine q for the acid-base reaction, assuming that the liquids have densities of 1.00 g/mL and the same heat capacities as pure water.
When 27.4 mL of 0.500 M H2SO4 is added to 27.4 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.) kJ/mol H2O
When a 3.13-g sample of liquid sulfuric acid dissolves in 33.6 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 22.00 oC to 41.81 oC. Calculate H in kJ/mol H2SO4 for the solution process. H2SO4(l) 2 H+(aq) + SO42-(aq) The specific heat of water is 4.18 J/g-K. Hsolution =____ kJ/mol H2SO4.
When a 7.46-g sample of solid sodium hydroxide dissolves in 36.9 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 24.00 oC to 68.26 oC. Calculate H in kJ/mol NaOH for the solution process. NaOH(s) Na+(aq) + OH-(aq) The specific heat of water is 4.18 J/g-K. Hsolution = . kJ/mol NaOH.
When 27.0 mL of 0.500 M H2SO4 is added to 27.0 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.) Answer: ______ kJ/mol H2O