Explain how the heat measured in example 5.5 diffees from enthalpy change for the exothermic reactions described by the following equation:
hcl + naoh ? nacl + h2o
reference example 5.5
heat produced by an exothermic reaction
when 50.0ml of 0.10 m hcl and 50.0 ml of 0.10 m naoh, both at 22.0c are added to a cofee cup calorimeter, the temperature of the mixture reaches a maximum of 28.9 c. what is the approximate amount of heat produced by this reaction
hcl + naoh ? nacl + h2o

What do you not know about it

Use the universal gas law formula: pv = nrt now, the key word in this problem is stp, so at stp, temperature will always be 0 degrees celsius and pressure will always be 1.0 atm or 760 torr. given something is at stp, we already know the two variables pressure and temperature. the other thing we can find with the given information is moles. to find moles, just divide grams by molar mass of the element. 16.0g / 2(16.00)g/mol = 0.5 moles plug the values in to the equation pv = nrt (1.0 atm)( x ) = (0.5 )(0+273=273k) the r value is just a constant for when we use atm, liters, moles and kelvin. i'm assuming you want your answer in liters, but if you dont just move the decimal 3 to the right in your final answer. so when plugging these numbers in to your calculator and trying to find x, you get 11.20665 liters using significant figures the answer is 11.2 liters