You add 7.326g of solid CaCl2 to 45.5 mL of water in a coffee cup calorimeter and measure as the temp. Increase from 22.6 C to 41.5 C. Specific heat water is 4.184 J/ g.C and the density of water is 0.9977 g/mL. Find the mass of water. PLEASE HELP ME!!!
Density = mass/Volume
solving for mass
mass = Density x Volume
mass = (0.9977g/ml(45.5-ml) = 45.3953 grams.
Are you sure 'mass of water' is all you needed? How about 'Heat of Reaction'?
q=mc(delta Temp)
q = (45.3953g)(4.184J/g-C)(41.5 - 22.6)C = 3589.7514joules
= 3590joules (3 Sig-Figs)
= 3.59Kj
I don't think you typed all of the problem/question.
You get mass H2O from mass = volume x density and that will answer your posted question.
However, most of these problems want to calculate delta H, usually in kJ/mol. That is done as follows:
q = mass H2O x specific heat H2O x (Tfinal-Tinitial)
Then delta H/g = q/7.326 g CaCl2.
delta H/mol = (q/7.326) x molar mass CaCl2. This will be in J/mol. Convert to kJ/mol.
To find the mass of water, we need to use the given information and apply the formula for density.
Density of water = mass of water / volume of water
Since the volume of water is given as 45.5 mL, we can substitute that into the formula:
0.9977 g/mL = mass of water / 45.5 mL
Now, let's solve for the mass of water by rearranging the equation:
mass of water = density of water * volume of water
mass of water = 0.9977 g/mL * 45.5 mL
mass of water = 45.33835 g
Therefore, the mass of the water in the coffee cup calorimeter is approximately 45.34 g.