Note that by % V proportional to % P I meant that % of total pressure the partial pressure is dependent on amount (in moles) of the substance and more is % volume for a constituent of mixture more will be the % of total pressure that its partial pressure will constribute. Don't confuse it with P proportional to 1/V we get for ideal gas law. Tha latter is true only for constant amount of substance.
Comment if you have any doubt.
At 380 C, the half-life period for the first order decomposition of HO, is 360 min....
The decomposition of ammonia gas is endothermic, AH = 92 kJ/mol. 2 NH3() = N2(g) + 3H2(g) What change to an equilibrium mixture of this reaction will result in the formation of more hydrogen gas? The addition of a catalyst. An decrease in temperature. An increase in volume. A decrease in the concentration of ammonia.
The decomposition of dimethyl ether at 504°C is a first order reaction with a half-life of 27.0 min. (CH₃)₂O(g) → CH₄(g) + H₂(g) + CO(g) A reaction vessel is charged with dimethyl ether at an initial pressure of 725 torr, and the reaction is initiated by rapidly heating the vessel to 504°C. Assuming a negligible time lag in beginning the reaction, what will the total gas pressure be in the vessel after 80.0 min? (assume ideal behavior)
6. (a) The rate constant for the first-order decomposition of N2Os in the reaction, 2 N2Os(g)-4 NO(g)+0.(g), k-3x10-s at 25°C. What is the half-life of N20s? What will be the pressure, initially 500 bar, at 10 min after initiation of the reaction? (b) Knowing the activation energy of the above reaction is 100 kJ mor', calculate the required reaction temperature at which the reaction rate is doubled. (c) What is the conversion efficiency of N20s at 1 bar and 25...
6. The decomposition of ammonia is: 2 NH (8) N2(8) 400 °C, what is the partial pressure of ammonia gas atm and H2(g) is 0.15 atm? 2 3(8) = N2(g) + 3 H2(g). If Kp is 1.5 x 103 at of ammonia gas at equilibrium when N2(g) is 0.10 7. A solution is prepared by dissolving 0.050 the solvent CCI. The total solution volume is 1.00L. When the pared by dissolving 0.050 moles of diiodocyclohexane, C6H1012(S), in al solution volume...
The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 → CH4 + H2 + CO is 3.2 x 10-4 5-1 at 450°C. The reaction is carried out in a constant-volume container. Initially, only dimethyl ether is present, and the pressure is 0.343 atm. What is the pressure of the system after 8.1 min? Assume ideal-gas behavior. 49) 0.29 x 0.44 atm
17. The decomposition of So,Cl, gas is a first order reaction with a half life of 2.3 x 10 seconds at 600K. If we begin with an initial partial pressure of SO,Cl, of 450 torr, what will be the partial pressure (in torr) of SO,Cl, after 150 hours? (A) 112 (B) 88 (C) 337 (D) 225 (E) 42
1) 2) 3) The decomposition of dinitrogen tetroxide to nitrogen dioxide at 400°C follows first-order kinetics with a rate constant of 3.84 X10-3-1. Starting with pure N204, how many minutes will it take for 38.0% to decompose? Suppose the surface-catalyzed hydrogenation reaction of an unsaturated hydrocarbon has a rate constant of 0.374 M/min. The reaction is observed to follow zero-order kinetics. If the initial concentration of the hydrocarbon is 2.90 M, what is the half-life of the reaction in seconds?...
1. The cartoon below represents the reaction of nitrogen gas (N2) with hydrogen gas (H2) to synthesize ammonia (NHs). Industrially, this che pro mical process is called the Haber-Bosch cess, and is still a very important reaction in the manufacture of fertilizers. The ability to fix every day). It has been estimated that use of nitrogen-based fertilizers has doubled the world's a. The cartoon below shows 6 molecules of hydrogen gas and 2 molecules of nitrogen nitrogen and manufacture fertilizers...
An isothermal (170 °C) isobaric (6 atm) catalytic gas-phase reaction is carried out in a fluidized CSTR: Assume that the reaction is elementary. The feed (benzene and hydrogen) is stoichiometric with θ。= 50-. The rate constant defined wrt benzene is 53 mol / (kgcat * min * atm) at 300 K with activation energy of 80 kJ/mol. What catalyst weight is required to reach 80% conversion? Hint: Use ideal gas law to relate pressure to concentrations (note the units of...
At 25°C the half-life for the first-order decomposition of a pesticide solution is 15.0 hrs. (a) Calculate the rate constant for the reaction. (b) If the starting concentration of pesticide is 0.500 M, what concentration will remain after 120 min at 25°C? neat handwriting, please!