I'm having trouble with a calorimeter question.
The heat of reaction is measured when 30.0 mL of 1 mol/L H2SO4(aq) is mixed together with 50.0 mL of 1 mol/L NaOH(aq)
I'm to assume the density and specific heat capacity for both is that of water.
initial temperature of NaOH = 24 degrees celsius
of H2SO4 = 24.4 degrees celsius
Final temperature = 32.9 degrees celsius
I'm supposed to calculate the molar heat of the reaction, and then calculate the percent difference in the value i found, and the universally accepted value of -57 kJ/mol
I am having troubles, as the number i recieve is much much lower than the widely accepted value, so i've decided i must be doing something wrong.
Please please help?
The heat of reaction is measured when 30.0 mL of 1 mol/L H2SO4(aq) is mixed together with 50.0 mL of 1 mol/L NaOH(aq)
I'm to assume the density and specific heat capacity for both is that of water.
initial temperature of NaOH = 24 degrees celsius
of H2SO4 = 24.4 degrees celsius
Final temperature = 32.9 degrees celsius
I'm supposed to calculate the molar heat of the reaction, and then calculate the percent difference in the value i found, and the universally accepted value of -57 kJ/mol
I am having troubles, as the number i recieve is much much lower than the widely accepted value, so i've decided i must be doing something wrong.
Please please help?