Calculate ΔE, and determine whether the process is endothermic or exothermic for the following cases. a. Calculate ΔE for a system that absorbs 661.0 kJ of heat from its surroundings and does 277.0 kJ of work on its surroundings.
b. Calculate ΔE, if q= 1.60 kJ and w= -657 J . Express your answer using two significant figures.
c. Calculate ΔE, if the system releases 56.5 kJ of heat while doing 13.0 kJ of work on the surroundings. Express your answer using three significant figures.

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.

lab safety rules

explanation: