Calculate the volume of oxygen necessary to form 39.0 g of sodium peroxide from sufficient sodium metal. (assume STP conditions)
Calculate the volume of oxygen necessary to form 39.0 g of sodium peroxide from sufficient sodium...
sodium peroxide (Na2O2) is used to remove carbon dioxide from (and add oxygen to) the air supply in spacecrafts. it works by reacting with CO2 in the air to produce sodium carbonate (Na2CO3) and O2. 2 Na2o2(s) + 2 CO2(g) > 2 Na2CO3(s) + O2(g) what volume (in liters) of CO2 can be consumed at STP by 715 g Na2O2?
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?
37.2 g of sodium metal and 23.7 L of chlorine react to form sodium chloride under STP condition. Identify the limiting reactant. What is the theoretical yield of sodium chloride when 37.2 g of sodium reacts with 23.7 L of chlorine at STP?
Student Number Soichiometry II Mass-Volume Calculations Lat Volume-Volume Calculations Part I: Mass - Volume 1. How many grams of sodium water? y grams of sodium metal are needed to generate 4.00 L of hydrogen (at STP) from What volume of hydrogen at 20°C and 800. mm Hg will be formed by the reaction of 20.0 g of calcium with an excess of hydrochloric acid 3. When water is decomposed by electrolysis, what volume of oxygen 25°C and 750. mm Hg...
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...
a) Calculate the volume at STP of a 4.000 L balloon filled with oxygen at 2.000 atm and 25.00 oC. b) How many moles of oxygen at STP? c) How many grams of oxygen at STP? d) Calculate the density of oxygen at STP using the volume from problem A and the mass from problem C e) Calculate the density of oxygen at STP using the molar volume, 22.414 L/mol.
(Part A) Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) → 2H2O(l) + O2(g) This reaction is accelerated by light, heat, or a catalyst. The concentrations of aqueous hydrogen peroxide solutions are normally expressed as percent by mass. In the decomposition of hydrogen peroxide, how many liters of oxygen gas can be produced at STP from 26.8 g of a 7.50% hydrogen peroxide solution? (Part B) What volume of bromine (Br2) vapor measured at 100.°C and 700. mmHg pressure would...
In an experiment. it is possible to calculate the moles of oxygen from either the volume formed at STP or from the weight of oxygen generated. Which gives the more accurate value? Why? Explain thee effect that failure to subtract the water vapor pressure from the total pressure would have on your determination of molar volume? (Would your molar volume be too high, the same, or too low and why?)
Part A Hydrogen and oxygen combine to form H,O via the following reaction: 2H2(g) + O2(g) → 2H2O(g) How many liters of oxygen (at STP) are required to form 14.9 g of H2O? Express the volume to three significant figures and include the appropriate units. HMÅ O ? VE Value Units Submit Request Answer