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    Gas Stoichiometry

    Gas Stoichiometry refers to the examination of the relative proportions of reactants and products in a chemical reaction involving gases. It is important to note that gas stoichiometry is only accurate when the gases and the physical conditions are assumed to be ideal, where the volume, pressure and temperature are known to be a fixed value. If the conditions are ideal, then the ideal gas law can be used to calculate any gas stoichiometry problem. The ideal gas law is commonly written as: PV = nRT, where P is the pressure of the gas V is the volume of the gas n is the amount of gas in moles R is the universal gas constant, which is 8.314 J*K^(-1)*mol^(-1) T is the temperature of the gas So if there are 0.5 moles of a certain gas, at 400 kpa and 300 Kelvin, then the volume of the gas can be calculated by substituting the values into the ideal gas equation: PV = nRT V = nRT/P = (0.5*8.314*300)/400 = 3.12 L of gas. Thus, understanding gas stoichiometry and the ideal gas law is crucial for predicting how a gas will react to varying physical conditions. © BrainMass Inc. brainmass.com May 24, 2024, 1:40 pm ad1c9bdddf

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    Pressure and Volume Change of a Gas

    I need some help in answering a question regarding caculations of how a compressed gas becomes a liquid: 10,000 m3 of natural gas as methane is the starting point at 288 Kelvin We are told that 2 things happen to the gas: 1) The 10000 m3 gas volume is compressed from 101 KPa to 6895 KPa I know this is PV =nRT but how

    Lab : Gases, Pressure and Stoichiometry

    Add 0.5g of sodium bicarbonate, NaHCO3 into a flask. Record the initial pressure and temperature in the flask. Add 10 mL of water to the flask to dissolve the NaHCO3 then record the pressure as the initial pressure for the experiment. Record the gas volume as the initial volume. Add 1 mL of 1M HCl, allow the temperature in the

    Density, Molar Mass and Stoichiometry

    1) Calculate the density of NO2 gas at 0.970 atm and 33C degree. 2) Calculate the molar mass of a gas if 2.50g occupies 0.885L at 685 torr and 33C degree. 3) Calcium hydride,CaH2 , reacts with water to form hydrogen gas: CaH2(s)+2H2O(l)>>Ca(OH)2(aq)+2H2(g) This reaction is sometimes used to inflate life rafts, weath

    Gas Laws and Stoichiometry

    1. A gas occupying a volume of 725mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final the volume? 2. The volume of a gas is 5.80L, measured at 1.00 atm. What is the pressure of the as in mmHG if the volume is changed to 9.65 L? (The temperature r

    Gas Laws, Stoichiometry and Enthalpy

    Question 1 A sample of a gas occupies 1.40 x 103 mL at 25oC and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg? 2,800 mL 2,100 mL 1,400 mL 1,050 mL 700 mL -------------------------------------------------------------------------------- Question 2 The gas pressure in an aerosol can

    One Mole of any gas occupies 22.4 L at STP

    Consider the following reaction, which takes place in an autoclave at 250C and 800 atm. 4NH3(g) + 7O2(g) = 4 NO2(g) + 6H2O(g) Into the reaction vessel has been placed 200L of NH3(g) and 120L of O2(g). The reaction is allowed to go to completion. Determine the quantity, in moles, of the gas that remains unreacted

    Commercial Air Bags

    Commercial automobile air bags use a spark to initiate the decomposition of solid sodium azide. NaN3 to nitrogen gas. How many grams of NaN3 must react to make 75.0 L of N2 at 1.oo atm? A. 14.6 g NaN3 B. 129 g NaN3 C. 1.14 x 10 TO THE POWER OF 3 g NaN3 D. 193 g NaN3 E. 145 g NaN3

    Atmosphere, Atomic weight, and Mass

    3. a.) The initial reaction when an automobile airbag deploys is: 2NaN3(s) → 2Na(s) + 3N2(g). If 125.0g of NaN3 reacts, how many liters of N2 gas result at 25.0oC and a pressure of 1.00 atmosphere? 3. b.) The recent death of a former soviet spy is attributed to the effects of an isotope of Polonium with an atomic

    applications of gas law

    See attached file for full problem description. 1. Gaseous CH4 reacts with O2 according to the following UNBALANCED equation: CH4 + O2 -->  CO2 + H2O What volume of oxygen at 20ºC and 97kPa is needed to react with 3.50 mol of CH4? 2. What volume of CO2 measured at 25ºC and 0.95atm is produced by the combusti

    Environmental chemistry question - short

    Assume that waste will contain 295.0 mg/L of biodegradable CH2O and will be processed through a 200000.0 L/day sewage treatment plant which converts 40% of the waste to CO2 and H2O. Calculate the volume (in Liters) of air (at 25 degrees C, 1 atm) required for this conversion. Assume that the O2 is transferred to the water with 2

    What volume of Cl2(g) at STP would you need to obtain a 250g sample of Cl2

    1. What volume of Cl2(g) at STP would you need to obtain a 250g sample of Cl2(g)? 2. A .418g sample of gas has a volume of 115mL at 66.3 degrees Celsius and 743mmHg. What is the molar mass of this gas? 3. What is the volume, in liters, occupied by a mixture of 15.2g Ne(g) and 34.8g Ar(g) at 7.15 atm pressure and 26.7 degre

    Niobium Converted to Niobium Hydride

    In one experiment, 0.780 g Nb (s) was sealed in a 28.0 mL glass tube at 25°C under 6.33 atm of hydrogen gas, H2. After reacting with the hydrogen for one week, all of the niobium had been converted to niobium hydride, NbH. Calculate the final pressure of hydrogen gas in the system at 25°C.

    Gas stoichiometry

    Calculate the mass in grams of Hydrogen chloride produced when 5.6 L of molecular hydrogen measured at STP react with an excess of molecular chlorine gas.