Achemical reaction was run in 210.0 ml of h2o. during the reaction, the temperature of the h2o changes from 27.2 oc to 57.6 oc. how much heat (in kj) did the chemical reaction produce? for h2o, cp= 4.184 j/(g · oc). assume the mass of the solution is 210.0 g. enter your answer as a positive decimal number.

 The quantity of heat produced by the reaction is +26710.656J

Explanation:

Quantity of Heat, Q = mass * specific heat capacity *temperature change

Q = mCpTc, where m= mass, Cp= specific heat capacity, Tc is temperature change

m= 210.0g, Cp=4.184J/(g · oC), Tc= 57.6 - 27.2 = 30.4 oC

Q = 210.0g *4.184J/(g · oC) * 30.4 oC

Q = +26710.656J

Therefore, the quantity of heat produced by the reaction is +26710.656J.

Note: Even though heat is given out by the system and is normally written as a negative value to indicate that heat is lost, the answer is written as a positive decimal number according to instruction.

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.