1
answer
0
watching
73
views
10 Nov 2019
A calorimeter contains 20.0 mL of water at 13.0 degree C. When 2.00 g of X ( a substance with a molar mass of 63.0 g/mol) is added, it dissolve via the reaction X(delta) + H2O(I) rightarrow X (aq) and the temperature of the solution increases to 29 0 degree C . Calculate the enthalpy change. Delta H, for this reaction per mole of X Assume that the specific heat and density of the resulting solution are equal to those of water (4.18 J /(g degree C) and 1.00 g /m L ] and that no heat is lost to the calorimeter itself, nor to the surroundings.
A calorimeter contains 20.0 mL of water at 13.0 degree C. When 2.00 g of X ( a substance with a molar mass of 63.0 g/mol) is added, it dissolve via the reaction X(delta) + H2O(I) rightarrow X (aq) and the temperature of the solution increases to 29 0 degree C . Calculate the enthalpy change. Delta H, for this reaction per mole of X Assume that the specific heat and density of the resulting solution are equal to those of water (4.18 J /(g degree C) and 1.00 g /m L ] and that no heat is lost to the calorimeter itself, nor to the surroundings.
Bunny GreenfelderLv2
12 Oct 2019