A system comprised of 2.100 Times 10^1 g of C0_2(g) cools from 155.0^degree C to 45.0^degree...
Heat Capacity of a Gas at Constant Pressure A system comprised of 7.900×101 g of H2(g) cools from 170.0°C to 35.0°C at a constant pressure of 4.5 atm. The molar heat capacity at constant pressure for H2(g) is 28.86 J K−1 mol−1. a) Calculate q. b) Calculate w. c) Calculate . d) Calculate . Note - for part a) I have tried -1.54*10^5 J, 1.54*10^5 J and -3.08*10^5 J (these are all wrong). I'm on my last try, please help!
Heat Capacity of a Gas at Constant Pressure A system comprised of 5.500x101 g of Ar(g) cools from 165.0°C to 30.0°C at a constant pressure of 3.0 atm. The molar heat capacity at constant pressure for Ar(g) is 20.80 J K-1 mol-1. Calculate q. 1pts Submit Answer Tries 0/5 Calculate w 1pts Submit Answer Tries 0/5 Calculate ΔΕ. 1 pts Submit Answer Tries 0/5 Calculate ΔΗ. 1pts Submit Answer Tries 0/5
Need work step by step please! Heat Capacity of a Gas at Constant Pressure A system comprised of 1.900x100 g of C2H6(9) cools from 180.0°C to 45.0°C at a constant pressure of 2.5 atm. The molar heat capacity at constant pressure for C2H6(9) is 52.92 J K-1 mol-1. Calculate q. 1 pts Submit Answer Tries 0/5 Calculate w. 1 pts Submit Answer Tries 0/5 Calculate ΔΕ. 1pts Submit Answer Tries 0/5 Calculate ΔΗ. 1pts Submit Answer Tries 0/5
How many moles of gas are there in a 45.0 L container at 25.0 degree C and 500.0 mm Hg? (R - 0.082 L Atm/ mol.K) Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0 degree C and 1.00 aim. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions w ill produce w hat volume of the CO_2 gas? The value of Delta H degree for the reaction below is -482 kJ. Calculate the...
Heat Evolved During Combustion and Heat Capacity of a Gas at Constant Pressure A. Consider the following reaction: 2 C2H2(g) + 5 O2(g) 4 CO2(g) + 2H2O(l) Use standard heats of formation from Zumdahl 'Chemical Principles' 8th ed. Appendix Four pp A19 - A21. a) How much heat is evolved when 1.440×101 moles of C2H2(g) is burned in excess oxygen. Answer to 4 sig figs. b) How much heat is evolved when 2.250×102 g of CO2(g) is produced from the...
6. A piece of 155.0 g aluminium metal at 120°C was placed in a constant pressure calorimeter of negligible heat capacity containing 300.0 g of water at 20°C. Calculate the final temperature of the system (the aluminium metal and the water) in °C: given the specific heat of aluminium metal = 0.90 J/g °C, and that of water 4.184 J/g °C
The following information is given for water at latm: boiling point = 100.0 degree C Delta H_vap(100.0 degree C) = 2.259xl03 J/g melting point = 0.000 degree C Delta H_fus(O.OOO degree C) = 333.5 J/g Specific heat solid = 2.100 J/g degree C specific heat liquid = 4.184 J/g degree C A 27.00 g sample of solid water is initially at -28.00 degree C. If 1.007xl04 J of heat are added to the sample at constant pressure (P = 1...
Use the Information given below, calculate the heat change of the system when 33.7 g of water at 32.5 degree C is converted to steam at 129.1 degree C. (C = specific heat capacity) Delta H_fusion for H_2O = 6.20 kJ/mol C_ice = 2.087 j/g degree C Delta H_vaporization for H_2O = 40.7 kJ/mol C_water = 4.184 J/g degree c molar mass H_2O = 18.01 g/mol C-steam = 1.966 j/g degree C (please include the appropriate sign in your answer)
Consider converting 1.50 mol of ice at - 25 degree C to liquid water at 55 degree C at 1 atm. What calculation would give the quantity of heat required by this process in J? The molar heat capacity of ice is 37.6 mol^-1 degree C^-1. The molar heat capacity of liquid water is 75.4 J-mol^-1 degree C^-1. The heat of fusion of water is 6.02 kJ mol^-1. (A) q = (1.50 mol) (6.02 kJ/mol) (1000 J/kJ) (B) q =...
The following reaction was allowed to come to equilibrium at 35 degree C. The initial molar concentration for SO_3 is 0.675 M ([SO_3| = 0.675 M) and the initial molar concentration for CO_2 is 0.444 M (|CO_2] = 0.444 M). After the reaction reached equilibrium the concentration of CO_2 now equals 0.214 M ((CO_2] = 0.214 M). What is the K_c value for the reaction? 0.00987 0.0342 7.31 11.8 16.7 At 35 degree C the equilibrium constant value (K_c) for...