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- Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 309. liters per second of dioxygen are consumed when the reaction is run at 217.°C and 0.70atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.An unknown gas, D, reacts with fluorine gas to form the compound DF4 (g), as represented by the following equation: D(g) + 2F 2 (g) --> DF4 (g) B. What is the initial rate of disappearance of F2 (g) in trial 1. Justify.Ammonium perchlorate (NH4ClO4) is a solid rocket fuel that was used in space shuttles. When heated at 200oC, it decomposes to a variety of gases, with the most important being N2(g), Cl2(g), O2(g), and H2O (g). Write a balanced chemical equation for the decomposition of NH4ClO4, assuming that only the products listed above are generated. The sudden appearance of hot gaseous products in a small initial volume leads to a rapid increase in pressure and temperature, which give the rockets its thrust. What total pressure of gas would be produced at 800 oC by igniting 7.00x105 kg of NH4ClO4 and allowing it to expand to a volume of 6.4x106L? (assume ideal gas behavior). Calculate the molar fraction of Cl2 and its partial pressure.
- 1) Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2(g) ® SO2(g) + Cl2(g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 liter bulb and the temperature is raised to 375K. (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375K. Note: Please answer both A and B1) Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2(g) ® SO2(g) + Cl2(g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 liter bulb and the temperature is raised to 375K. (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375K. (c) Give the expression for the equilibrium constant (either Kp or Kc) for the decomposition of SO2Cl2(g) at 375K. Calculate the value of the equilibrium constant you have given, and specify its units. (d) If the temperature were raised to 500K, what effect would this have on the equilibrium constant? Explain briefly. Note: Please answer just C and D. Thank you.Charles’s law states that if the pressure of a dry gas is held constant, then the volume V of the gas and its temperature T, measured in degrees Kelvin, satisfy the relationship V=cT, where c is a constant. Which of the following best describes the relationship between the rate of change, with respect to time t, of the volume and the rate of change, with respect to time t, of the temperature? a. dV/dt=T(dc/dt) b.dV/dt=c(dT/dt) c.dV/dT=c d. 1=c(dT/dV)
- p=pRT is the perfect gas equation where p is pressure, p is density T temperature and R is constant. Solve for the rate of change in pressure if the rate of change in density and temperature are 12 and 5, respectively.Give the theoretical forward rate equation when all are gases except water4 PH3 + 2 H2 + 9 O2 D 2 P2O5 + 8 H2O(liq) + 25 kJa) when PH3 is a gas, rate = kf [b) when PH3 is a liquid, rate = kf [In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction is now the first step taken to make most of the world's fertilizer. Suppose a chemical engineer studying a new catalyst for the Haber reaction finds that 322. liters per second of dinitrogen are consumed when the reaction is run at 286.°C and 0.16atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.
- Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 965 liters per second of dioxygen are consumed when the reaction is run at 216°C and 0.58 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.Use the kinetic theory to justify the following observations: (a) the rate of a reaction in the gas phase depends on the energy with which two molecules collide, which in turn depends on their speeds; (b) in the Earth’s atmosphere, light gases, such as H2 and He, are rare but heavier gases, such as O2, CO2, and N2, are abundant.The highest building in Montreal is the ‘1 square building’, with a height of 203m.The atmospheric pressure in the streets of Montreal is P1 = 9.9 x 104Pa.Suppose air density is constant : ρair= 1,2 kg/m3 and g = 9.8 m/s2. Suppose the rooftop temperature to be T = 298K, and the air composition is 100%N2 molecules. The collision cross-section of N2 molecules is 0.43 nm2.*f. Find the collision frequency. Is it in the order of magnitude that you wereexpecting?