You placed 6.35 g of a mixture containing unknown amounts of BaO(s) and MgO(s) in a 3.50-L flask containing CO₂(g) at 30.0°C and 750. torr. The solid BaO and MgO in the flask completely reacted to form BaCO₃(s) and MgCO₃(s), respectively. After the reactions to form BaCO₃(s) and MgCO₃(s) were completed, the pressure of CO₂(g) remaining was 255 torr, still at 30.0°C. Calculate the mass of BaO(s) in the initial mixture in grams. (Assume ideal gas behavior).

A weather balloon is inflated to a volume of 29.8 L at a pressure of 753 mmHg and a temperature of 25.3 ∘C. The balloon rises in the atmosphere to an altitude where the pressure is 390. mmHg and the temperature is -16.7 ∘C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

Please don't provide handwritten solution

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)

In a collision of sufficient force, automobile air bags respond by electrically triggering the explosive decomposition of sodium azide (NaN3) to its elements. A 69.9−g sample of sodium azide was decomposed, and the nitrogen gas generated was collected over water at 26°C. The total pressure was 748.5 mmHg. How many liters of dry N2 were generated?

The chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is 2CH, (g) +3 Cl, () 2CH,CI(g) + 2 HCI(g) + 2CI (g) Suppose that a chemist combines 273 mL of methane and 689 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K. If the reaction reaches 75.0% completion, what is the total pressure in the flask? Pictal = atm What is the partial pressure of CH,? Pon, = atm What is the partial pressure of Cl, ?

You placed 6.35 g of a mixture containing unknown amounts of BaO(s) and MgO(s) in a 3.50-L flask containing CO₂(g) at 30.0°C and 750. torr. The solid BaO and MgO in the flask completely reacted to form BaCO₃(s) and MgCO₃(s), respectively. After the reactions to form BaCO₃(s) and MgCO₃(s) were completed, the pressure of CO₂(g) remaining was 205 torr, still at 30.0°C. Calculate the mass of BaO(s) in the initial mixture. (Assume ideal gas behavior).

You set up a reaction with Gallium metal in excess hydrochloric acid at 28 degrees Celsius. It reacts in the following: 2Ga(s)+6HCl(aq)→2GaCl3(aq)+3H2(g) You collect 157 mLs and 0.951 atm of hydrogen over water. How many moles of Ga reacted? The partial pressure of water at 28 degrees is 0.0372 atm.