In order to determine the rate of photosynthesis (the conversion by plants of carbon dioxide and water into glucose and oxygen), the oxygen gas emitted by an aquatic plant is collected over water at a temperature of 293 K and a total pressure of 755.2 mmHg. Over a specific time period, a total of 1.02 L of gas is collected. What mass of oxygen gas (in grams) forms?

If there are 1.5 x 109 cows each "passing" on the average 240. Liters of CH4 (g) per day, in one day if all of that CH4 were to be safely collected and undergo a controlled but complete combustion reaction, how many grams of CO2 would contribute to the Greenhouse effect of the Earth?   You will first need to have the combustion reaction of CH4. Make an assumption that the Temperature of the collected gas is 22.4 L = 1 mol, STP conditions (which it really is not at).

A reaction at 19.0°C evolves 483.mmol of carbon dioxide gas. Calculate the volume of carbon dioxide gas that is collected. You can assume the pressure in the room is exactly 1atm . Be sure your answer has the correct number of significant digits.

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 21.0 cm wide and 25.2 cm high. The maximum safe pressure inside the vessel has been measured to be 8.80 MPa. For a certain reaction the vessel may contain up to 0.650 kg of carbon dioxide 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: I °C

A reaction at 34.0 °C evolves 174. mmol of carbon monoxide gas. Calculate the volume of carbon monoxide gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits. volume: L x10

A gas system has initial volume and moles of 7.56 L and 0.537 moles. If the volume changes to 8.93 L, under conditions P and T, determine the number of moles.

Calculating the reaction rate of one reactant from that of another The reform reaction between steam and gaseous methane (CH,) produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. Synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen. Suppose a chemical engineer studying a new catalyst for the reform reaction finds that 373. liters per second of methane are consumed when the reaction is run at 216. °c and the methane is supplied at 0.60 atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. kg |x10 S

A car tire is inflated at a temperature of 12.0 Celsius, 2.45 ATM and a volume of 11.8 L. The tire heats up during driving resulting in a temperature of 65.0 Celsius and a volume of 12.2 L. If normal Tire pressure is 2.00- 3.20 ATM, determine the tire pressure and effect of the new pressure on the tires?

2. Olympic cyclists fill their tires with helium to make them lighter. The mass of air used in the air filled tire is 8.56 g. Assume that the volume of the tire is 855 mL, that it is filled to a total pressure of 8.51 atm, and that the temperature is 25°C. a. Calculate the mass of helium in a helium-filled tire. (you must show all work to earn full credit). b. What is the difference between the two? c. Why is the helium-filled tire lighter?

A reaction between liquid reactants takes place at - 14.0 °C in a sealed, evacuated vessel with a measured volume of 40.0 L. Measurements show that the reaction produced 36. g of chlorine pentafluoride gas. Calculate the pressure of chlorine pentafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Be sure your answer has the correct number of significant digits. pressure: |II atm