(6 pts.) 1. The air pressure in the inner tube of a tire on a typical...
(6 pts.) 1. The air pressure in the inner tube of a tire on a typical racing bike is held at a pressure of 115 psi (pounds per square inch). Convert this pressure to atm and mm Hg. (3 pts. each) 2. The atmospheric pressure is 0.975 atm. Determine the pressure of the enclosed gas in each of the cases depicted below. 80 47 mm mm Gas Gas (6 pts.) 3. A 4.00 L flask contains 9.00 g of Ne...
19. Calculate the rate of flow of O, (g) through the walls of a porous tube if H, (g) flows at the rate of 3.95 x 10 mL/sec under identical conditions. 20. Acetylene gas reacts with oxygen gas as follows: 2 C,H, (B)+5 0, (8) 4 CO, (B) +2 H,0 (g) What quantity of CO, (g) is formed when 6.0 L of acetylene gas is completely combusted? 21. How many liters of O,(g) at STP are evolved when 3.25 g...
i need help with the last four questions along with step by step he appropriate gas law to solve questions 1-6. Show work. (2 pts) A certain amount of a gas at a constant temperature has a pressure of 5.50 atm and a volume of 10.0 mL. If the volume is decreased to 125.0 mL, what is the resulting pressure of the gas? : 924 a4m 125 O P v (2 pts) If 0.722 L of a certain gas at...
given this electrochemical cell: Concentration of H+ is unknown, Pressure of H2 is constant at 1 atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+ half-cell acting as the cathode. a) write out the oxidization and reduction half reactions, and the overall chemical reaction occurring, and find the initial pH in the H+ | H2 | Pt cell b) What is the equilibrium constant of the reaction happening in the cell? Tl(s) | Tl*(aq, 0.50 mol...
*** ** -305.01 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 AHºf (kJ/mol) AG°f (kJ/mol) Sº (/mol K) 0 205.1 Oxygen 02 (g) O(g) 03 (g) 249.2 231.7 161.1 142.7 163.2 238.9 Phosphorus AH° (kJ/mol) AG°f(kJ/mol) sº (/mol K) Nitrogen AH°(kJ/mol) AG°f(kJ/mol) s° /mol K) N2 (8) 0 191.6 N (g) 472.7 455.6 153.3 NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 132.0 -79.0 113.0 90.3 86.6 210.8 51.7 66.1 261.8 NH4+ (aq) NO (g) NOCI (9) NO2 (g)...
1. 2. * Incorrect. What is the heat of formation of elements in their standard states? Did you use the correct equation of products minus reactants? The amino acid glycine, C2H5NO2, is one of the compounds used by the body to make proteins. The equation for its combustion is 4C2H5NO2(s) + 902(g) + 8C02(g) +10H20(1) +2N2(0) For each mole of glycine that burns, 973.49 kJ of heat is liberated. Use this information, plus values of AHF for the products of...
6) (3 pts) A sample gas is composed of four components. The gas molecules in the picture below are representative of the overall concentrations in the sample. If the total pressure of the gas mixture is 4.0 atm, what is the partial pressure of gas A? = gas A gas A The partial pressure of (3 pts) Water has a vapor pressure of 0.30 atm at 340 K. What is the density of water vapor (g/L.) under these conditions? Dem...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction Ng(8) + 3 H (8)=2 NH (8) the standard change in Gibbs free energy is AG° = -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.450 atm, P, = 0.250 atm, and PH, = 0.950 atm? kJ/mol AG -
Using enthalpies of formation (Appendix C), calculate ΔH ° for the following reaction at 25°C. Also calculate ΔS ° for this reaction from standard entropies at 25°C. Use these values to calculate ΔG ° for the reaction at this temperature. COCl2(g) + H2O(l ) h CO2(g) + 2HCl(g). Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kW/mol) 0 AG: (kJ/mol) 0 S° (J/mol-K) 20.87 ΔΗ, (kJ/mol) -946.3 - 33422 AG; {kj/mol) --859,3 -2793 (J/mol-K)...
Question 1 1 pts Calculate AG at 25 °C, in kJ, f or the following reaction, at Fe 0.82, PH2-1.668 (atm), and[H] 0.339 M. Fe(s) 2H (aq) Fe2H2(g) ΔGo for Fe2+--78.9 kJ/mol