i really need help with my hw if people can help lead me to the answer it would be really helpful. so far i was only able to do number 1 1) If 2.00 mol of an ideal gas, initially at 1.53 atm and 280 K, is allowed to expand isothermally under a constant external pressure of 0.920 atm until the final internal pressure is 0.920 atm, what is the work done? my answer: -2368 J 2) If the gas involved is ideal and the process is reversible, obtain an expression for w (work), using our ‘regular’ thermodynamic variables, P, V, n, and T. 3) For which of these systems is the system’s energy conserved in every process: (a) a closed system; (b) an open system; (c) an isolated system; (d) a system enclosed in adiabatic walls? Please provide a brief explanation for your answer. 5) We showed ΔH = q for a constant-pressure process. Consider a process in which P is not constant throughout the entire process, but for which the final and initial pressures are equal. Need ΔH be equal to q here? (Hint: One way to answer this is to consider a cyclic process) 6) A sample consisting of 1.00 mol of a monatomic perfect gas (for which CV,m = 3/2R) is taken through the cycle shown below. (a) Determine the temperatures at 1, 2, and 3; (b) Calculate q, w, ΔU, and ΔH for each step and the overall cycle. If a numerical answer cannot be obtained, then write +, -, or ? as appropriate. 7) 2.50 mol of an ideal gas with CV,m = 12.47 J mol-1 K-1 is expanded adiabatically against a constant external pressure of 1.00 bar. The initial temperature and pressure of the gas are 325 K and 2.50 bar, respectively. The final pressure is 1.25 bar. Calculate the final temperature, q, w, ΔU, and ΔH.