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 394. liters per second of dinitrogen are consumed when the reaction is run at 209. °C and the dinitrogen is supplied at 0.45 atm. 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. kg 0 X S E C

When limestone (solid CaCO,) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete- the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 500. L. and heated to 520.0 °C. When the amount of CaCO, has stopped changing, it is found that 3.84 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO, and CaO at 520.0 °C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K, does not match the accepted value.

In order to produce solid iron, it first must bc processed from its orc, Fe2O1, in a blast furnace. During operation, CO gas (flue gas) is introduced into the furnace at 1650 °C and a pressure of 250 kPa. In this process flue gas reduces iron to its elemental form in the following reaction: 41. Fe;O30) COg Fe+ COz At one point in this process 256.0 L of CO was used to reduce iron ore. Assuming a complete reaction, how many grams of solid iron can be produced. Balanced chemical equation: Mass of Fe (in grams)

The human body burns glucose (C6H12O6) for energy according to this chemical reaction: C6H12O6+6O2→ 6CO2+6H2O The products of the reaction are carbon dioxide CO2 and water H2O Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mL of air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50kg  of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0 kg/m^3 .

A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder tha measures 52.0 cm wide and 62.4 cm high. The maximum safe pressure inside the vessel has been measured to be 7.00 MPa. For a certain reaction the vessel may contain up to 25.8 kg of sulfur hexafluoride gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Round your answer to 3 significant digits. temperature: C x10 X

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The nitrogen content of organic compounds can be determined by the Dumas method.The compound in question is first passed over hot CuO(s): Compound  N2(g) + CO2(g) + H2O(g) The gaseous products are then passed through a concentrated aqueous KOH solution to remove the CO2.The remaining gas contains N2 and water vapor.A 0.127-g sample of a compound was treated as above, producing 89.0 mL of N2 saturated with water vapor at 25 °C and 739.3 torr.What is the mass percent of nitrogen in the compound? . The vapor pressure of water at 25 °C is 23.8 torr.

Three bulbs are connected by tubing, and the tubing is evacuated. The volume of the tubing is 49.0 mL The first bulb has a volume of 58.0 ml and contains 6.07 atm of argon, the second bulb has a volume of 250 ml. and contains 1.62 atm of neon, and the third bulb has a volume of 27.0 ml. and contains 7.72 atm of hydrogen. If the stopcocks (valves) that isolate all three bulbs are opened, what is the final pressure of the whole system in atm? Answer:

A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder that measures 26.0 cm wide and 31.2 cm high. The maximum safe pressure inside the vessel has been measured to be 2.40 MPa. For a certain reaction the vessel may contain up to 0.237 kg of dinitrogen monoxide gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Round your answer to 3 significant digits. temperature: || °C Contacts G.. APR 24 80 888 F2 DII F3 F4 F7 F8 F9 F10

205L of carbon dioxide at STP is compressed and then dissolved in 10.0L of water. What is the molar concentration of teh resulting solution?