How many milliliters of CO gas would be produced by the complete reaction of 2.40 g of C at STP according to the following reaction? Remember 1 mol of an ideal gas has a volume of 22.4 L at STP     C(s) + H₂O(g) → CO(g) + H₂(g)

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A sample contains 2.0 moles of He gas and 6.0 moles of Ar gas. What is the mole fraction of He gas (XHe)? 0.33 0.75 0.25 2.0

A hot air balloon is filled with 1.13×106 L of an ideal gas on a cool morning (11°C). The air is heated to 121°C volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon. Do not give handwriting solution.

A gaseous compound has a density of 1.68 g/L at 21.2 °C and 1.30 atm. What is the molar mass of the compound? molar mass: g/mol

What volume in liters will 1 mole of ideal gas occupy under at STP? 44.651 L 22.414 L O24.465 L 0002241 D Question 7 Which of the following is a true statement? Oceans are naturally acidic and becoming more acidic as the concentration of CO₂ in the atmosphere increases Oceans are naturally alkaline and becoming more acidic as the concentration of CO₂ in the atmosphere increases Oceans are naturally pH-neutral and becoming more alkaline as the concentration of CO₂ in the atmosphere increases None of the above. D Question 8 Acid rain is caused by which of the following compounds? Carbon dioxide and sulfur dioxide Sulfur dioxide and nitrogen oxides O Carbon monoxide and nitrogen axides None of the above D Question 9 Chesapeake Bay's poor health is mostly a result of pollution with the following Radionuclides Nutrients Pathogens O Volatile Organic Compounds

In the reaction 2 KCIO3(s) →→→ 2 KCI(s) + 30₂(g) how many liters of oxygen gas, O₂, measured at STP are produced from the decomposition of 395 g of potassium chlorate, KCIO3 ? V = 104.5 Incorrect L

2.75 g of an unknown gas at STP fills a 500. mL flask. What is the molar mass of the gas? g/mol 1 2 3

Find the volume of O2 (at STP) formed when 33.4 g of KClO3 decomposes according to the following reaction.  molar mass for KClO3 is 122.55 g/mol. 2 KClO3(s)  →  2 KCl(s) + 3 O2(g)