E2B.3(b, The constant-pressure heat capacity of a sample of a perfect gas was found to vary with temperature according to the expression C/(JK") = 20.17 + 0.4001(T/K). Calculate q, w, AU, and AH when the temperature is raised from 25°C to 100°C (i) at constant pressure, (ii) at constant volume.

3. Derive the thermodynamic equation of state for an ideal gas starting from internal energy then express this equation in a form without differentials. = -P +T| T LƏT.

Benzoic acid, C;HsO:H, is typically used as a çalibrant for determining the specific heat of bomb calorimeters. It combusts via the following unbalanced chemical reaction: C,H5O2H (s) + 02(g) → CO2 (g) + H2O(1) 3. For this experimental setup and reaction, the constant volume heat flow is known to be gy = -26.979 kJ. Over the course of the reaction, the temperature rose from 19.863 °C to 22.540 °C. Calculate the heat capacity, Cou, for this calorimeter in kJ °C-!.

Suppose a piece of solid lead weighing 41.3 g at a temperature of 312 °C is placed in 413 g of liquid lead at a temperature of 374 °C. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is AH fus = 4.77 kj mol¹ at its melting point of 328 °C, and the molar heat capacities cp of solid and liquid lead are 26.9 and 28.6 J K¹ mol-¹, respectively. (Enter your answer to three significant figures.) T₁= Jc Submit Answer Try Another Version 1 item attempt remaining

1. The specific heat capacities (in units of J/g-K) of V, W, and Zn are 0.489, 0.132, and 0.388, respectively. What is the order of the molar heat capacities? Formula weights: V 50.94; W 183.8; Zn 65.4 (c) W>V>Zn (a) V>W>Zn (d) W>Zn>V (b) V>Zn>W (e) Zn>V>W

Q3) Thermodynamic Processes- 2.0 mol of a diatomic ideal gas undergoes a process in which it is compressed very slowly from state a (V. = 3.0 m³, P, = 1000 Pa) to state b (V, = 1.0 m³), in such a way that the system maintains thermal equilibrium with its surroundings at all times. P (Pa) 3000 2000 A. Find the change in internal energy during the process. 1000 B. Find the final pressure of the gas. 1 3 4 V(m³) C. Find the work done by the piston on the gas during this process. (Hint: Since Pis not constant during this process, it doesn't come out of the integral. Use the ideal gas law to find an expression for Pin terms of constants and the integration variable V) D. So what's the work done by the gas on the piston during this process? E. How much heat – if any - was transferred between the gas and surroundings during this process? Did heat flow from the gas to the surroundings or from the surroundings to the gas? Explain your reasoning. F. At the end of the process, is the average…

(a) Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2. Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units.  (b)Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K.  (c) Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.

A quantitity of 100mL of 0.500 MHCl was mixed with 50 mL of 0.500M NaOH in a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and NaOH solutions was the same, 20ºC, and the final temperature of the mixed solution was 22.3ºC. Calculate the heat change for neutralization reaction on a molar baisis.