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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.

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

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

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

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

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.