In a constant‑pressure calorimeter, 55.0 ml55.0 ml of 0.320 m ba(oh)20.320 m ba(oh)2 was added to 55.0 ml55.0 ml of 0.640 m hcl.0.640 m hcl. the reaction caused the temperature of the solution to rise from 21.72 ∘c21.72 ∘c to 26.08 ∘c.26.08 ∘c. if the solution has the same density and specific heat as water ( 1.00 g/ml1.00 g/ml and 4.184j/g⋅k,)4.184j/g⋅k,) respectively), what is δδh for this reaction (per mole h2oh2o produced)? assume that the total volume is the sum of the individual volumes.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

while cooking a piece of 1/2 pound beef steak, a cast iron pan (2.4kg in weight) was heated 260 celsius.