sodium peroxide (Na2O2) is used to remove carbon dioxide from (and add oxygen to) the air...
Sodium peroxide is often used in self-contained breathing devices such as those used in fire emergencies because it reacts with exhaled carbon dioxide to form sodium carbonate and oxygen gas: a. balance the equation ___ Na2O2(s) + _____ CO2 (g) ----> _____ Na2Co3 (s) + O2 (g) b. If you begin with 3.50 g of Na2O2, how many moles of Na2O2 is that? c. If you begin with 3.50 g of Na2O2, how many moles of )2 can be produced...
1) If 1.63 g of sodium peroxide (Na2O2) react with water to produce sodium hydroxide and oxygen, how many liters of oxygen will be produced at 25.0 °C and 725 torr? 2 Na2O2(s) + 2 H2O(l) → 4 NaOH(aq) + O2(g) Liters of oxygen = 2) A gas occupies a volume of 5.87 L at 0.950 atm. At what pressure will the volume be 8.45 L? Pressure =
2 NA+O2=Na2O2. A. Calculate the theoretical yield of sodium peroxide, Na2O2, if 61.0 g of sodium reacts with excess oxygen. B. When this reaction was carried out in the lab, 85.7 g of Na2O2 was obtained. What is the percent yield of Na2O2?
Sodium peroxide Na2O2 decomposes as follows: 2Na2O2(s) = 2Na2O(s) + O2(g). Find the mass of Na2O2 (molar mass 77.98 g/mol) required to produce 78.4 L of O2(g). Assume ideal-gas behavior of O2(g) and its molar volume 22.4 L/mol. (A) 22.3 g (B) 45.0 g (C) 273 g (D) 546 g (E) 1092 g
Sulfuric acid and sodium carbonate react to form carbon dioxide, water, and sodium sulfate as shown in the balanced equation below: H2SO4(aq) + Na2CO3(s) + CO2(g) + H2O(1) + Na2SO4(aq) In the presence of excess sulfuric acid, how many moles of CO2 would be released if you have 12.50 g of Na2CO3(s)? The molar mass of sodium carbonate is 106.0 g/mol, the molar mass of sulfuric acid is 98.08 g/mol, and the molar mass of carbon dioxide is 44.01 g/mol....
Upon heating, sodium bicarbonate decomposes into sodium carbonate, carbon dioxide, and water vapor according to the following chemical reaction: 2 NaHCO3 (s) →→ Na2CO3 (s) + CO2 (g) + H2O (g) If the initial mass of sodium bicarbonate is 4.859 g, how much sodium carbonate should be produced? a. 3.066 g b. 2.211 g c. 6.131 g d. 4.859 g
Strontium carbonate decomposes into strontium oxide and carbon dioxide gas when heated, as shown below. What mass of strontium carbonate would be required to produce 1.349 g of strontium oxide, assuming the reaction went at 100% yield? 2. SrCOs(s)->SrO(s)+ CO2 (g) What volume of oxygen, in mlL, would be produced at STP (0 °C and 1.00 atm) by the decomposition of 3.428 g of sodium chlorate, according to the equation below? 3. 2 NACIO,(s)->2 NaCl (s) + 3 O2(g) If...
Ethane is burned in air (oxygen) to form carbon dioxide and water by the following reaction. Determine the maximum grams of carbon dioxide that can be formed if 57.9 g of ethane are reacted with 57.9 g of oxygen. 2 C2H6 + 7 O2 = 4 CO2 + 6H2O.
Part II : Volume - Volume 1. Carbon monoxide burns in oxygen to form carbon dioxide. What volume of oxygen at 25°C and 760. mm Hg is required to react with 15.0 L of carbon monoxide (at STP)? 2. What volume of hydrogen and nitrogen are required to produce 20.0 L of ammonia (all gases at STP)? 3. Acetylene ( CH) burns in oxygen to form carbon dioxide and water. How many liters of oxygen (at STP) are needed to...
In the reaction, CaCO3(s)⟶CaO(s)+CO2(g) how many liters of carbon dioxide, CO2, measured at STP, would be produced from the decomposition of 309 g of calcium carbonate, CaCO3?