A weather balloon is filled with 138.2 L helium at sea level where the pressure is 1.000 atm at 20.0 °C. After ascending until the pressure is 95.00 mmHg, the balloon expands to 750.0 L and bursts. What is the temperature (in K) at which the balloon bursts?

A 6.28L sample of methane was collected over water at 15°C until the pressure in the flask was 711 torr. A small amount of CaSO4(s) was then added to the flask to absorb the water vapor (forming CASO4-2H2O(s)). What is the pressure inside the flask once all the water is absorbed? Assume that the addition of CaSO4(s) absorbed all the water and did not change the volume of the flask. The pressure in the flask is i torr. How many moles of CH4(g) have been collected? i mol Attempts: 0 of 15 used Submit Answer Save for Later S DEC étv MacBook Air DD 80 F7 F8 F9 F10 F4 F5 F6 F3

The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4240 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)

A balloon is partly inflated with 4.50 liters of helium at sea level where the atmospheric pressure is 992 mbar. The balloon ascends to an altitude of 3.00× 103 meters, where the pressure is 853 mbar. What is the volume of the helium in the balloon at the higher altitude? Assume that the temperature of the gas in the balloon does not change in the ascent. L

A student adds 3.00 g of dry ice (solid CO2) to an empty balloon. What will be the volume of the balloon at STP after all the dry ice sublimes (converts to gaseous CO2)?

Liquid nitrogen trichloride is heated in a 3.00-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 858 mmH at 94°C. What is the mass of the original sample?

A weather balloon is inflated to a volume of 26.4 L at a pressure of 740. mmHg and a temperature of 27.1°C. The balloon rises in the atmosphere to an altitude where the pressure is 400. mmHg and the temperature is -13.1 °C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude. ? Viballoon L

Hw.75.

(Incorrect) Consider the reaction below P4(g) + 6 Cl₂(g) → 4 PC13(g) If 0.246 moles of P4 is mixed with 0.354 moles of Cl₂ in a 9.77-L rigid reaction vessel, what is the final pressure in the vessel after the reaction goes to completion? The final temperature is 350. °C. Assume 100% yield. 2.89 atm 1.24 atm (Your answer) 0.694 atm 2.21 atm (Correct answer) 5.15 atm