The dissolution of X is exothermic since T increased. What was q?
q = mass H2O x specific heat H2O x (Tfinal-Tinital)
Then q = delta H and that is negative.
That is delta H/1.97 g and you convert that to mols by
(-dH/1.97g) x 141 g/mol = -dH/mol. Post your work if you get stuck.
(DrBob222 please help me)
A sample of 1.97 grams of Z is dissolved into
500 grams of water which is in a styrofoam
coffee cup. The temperature is monitored and
is found to rise from 25.015◦C to 25.484◦C.
What is ∆Hsolution for substance Z? Assume
no heat is lost/gained by the cup itself. The
specific heat of water is 4.184 J/g·
◦C and the
molecular weight of Z is 141 g/mol.
Answer in units of kJ/mol of Z.
PLEASE DO NOT ROUND OR USE SIG FIGS
1 answer
1 answer