Gas Stoichiometry

Key Questions

• What is gas stoichiometry?

  Gas stoichiometry is the study of the relative amounts of reactants and products in reactions that involve gases.

  EXAMPLE
  Calculate the volume of gaseous NO₂ produced by the combustion of 100 g of NH₃ at 0°C and 100 kPa.

  Solution

  Step 1. Write the balanced chemical equation.

  4NH₃(g) + 7O₂(g) → 4NO₂(g) + 6H₂O(l)

  Step 2. Convert mass of NH₃ → moles of NH₃ → moles of NO₂.

  100 g NH₃ × #(1"mol NH"_3)/(17.03"g NH"_3) × (4"mol NO"_2)/(4"mol NH"_3)# = 5.872 mol NH₃ (3 significant figures +
  1 guard digit)

  Step 3. Use the Ideal Gas Law to calculate the volume of NO₂.

  #PV = nRT#

  #V = (nRT)/P = (5.872"mol" × 8.314"kPa·L·K"^-1"mol"^-1 × 273"K")/(100 "kPa")# = 133 L

  

  Ernest Z. · · Aug 29 2014

• How do you apply gas stoichiometry?
• How do you solve a gas law stoichiometry problem?
• How do you do gas stoichiometry problems at STP?
• When an AgNO3 solution is treated with 50.0 mL of HI gas to give 0.235 g of AgI, what is the temperature of the HI gas?
• When 10.0 mL of AgNO3 solution is treated with excess amount of HI gas to give 0.235 g of AgI, what is the concentration of the AgNO3 solution?
• Hydrogen sulfide reacts with sulfur dioxide to give H2O and S, H2S + SO2 = H2O + S(solid), unbalanced. If 3.0 L of H2S gas at 760 torr produced 4.8 g of sulfur, what is the the temperature in Celsius?
• If 100 mL of HCl gas at 300 K and 200 kPa dissolved in pure water requires 12.50 mL of the NaOH solution to neutralize in a titration experiment, what is the concentration of the NaOH solution?
• If 100 mL of HCl gas at 300 K and 100 kPa dissolved in pure water requires 12.50 mL of the NaOH solution to neutralize in a titration experiment, what is the concentration of the NaOH solution?
• If 100 mL of HCl gas at 300 K and 100 kPa dissolve in 20 mL of pure water, what is the concentration?
• When 2.00 g mixture of Na and Ca reat with water, 1.164 L hydrogen was produced at 300.0 K and 100.0 kPa. What is the percentage of Na in the sample?
• A 3.66-g sample containing Zn (at.wt. 65.4) and Mg (24.3) reacted with a dilute acid to produce 2.470 L H2 gas at 101.0 kPa and 300 K. What is the percentage of Zn in the sample?
• Hydrogen sulfide reacts with sulfur dioxide to give H2O and S, H2S + SO2 = H2O + S(solid), unbalanced. If 6.0 L of H2S gas at 750 torr produced 3.2 g of sulfur, what is the temperature in Celsius?
• A 5.0-L air sample containing H2S at STP is treated with a catalyst to promote the reaction, H2S + O2 = H2O + S(solid). If 3.2 g of solid S was collected, what is the volume percentage of H2S in the original sample?
• If 500 mL of HCl gas at 300 K and 100 kPa dissolved in pure water requires 12.50 mL of the NaOH solution to neutralize in a titration experiment, what is the concentration of the NaOH solution?
• If 500 mL of HCl gas at 300 K and 100 kPa dissolve in 100 mL of pure water, what is the concentration?
• Can the ideal gas law be made more precise?
• What are some common mistakes students make with gas stoichiometry?
• What are some examples of gas stoichiometry?
• What is gas stoichiometry?
• Question #73939
• Question #cffa0
• Question #9f7a6
• Question #97b37
• Question #301e2
• Question #764c2
• Question #4e869
• Question #bba7c
• Carbon monoxide burns : #sf(2CO+O_2rarr2CO_2)#. If you have 1 litre of #sf(CO)# how much #sf(CO_2)# is formed and how much #sf(O_2)# is required ?
• Question #9140f
• Question #faabd
• At #"1.20 atm"#, and a temperature of #"27"^@"C"#, #"75.0 L NH"_3"# gas is produced by the reaction between #"N"_2"# gas and #"H"_2"# gas. How many moles and what volume of #"N"_2"# and #"H"_2"# are required to produce #"75.0 L NH"_3"#?
• Question #744bf
• Calculate the volume of hydrogen required for complete hydrogenation of 0.25 #dm^3# of ethyne at STP?
• Given the reaction N2 + 3H2 -->2NH3, what volume of hydrogen is necessary to react with five liters of nitrogen to produce ammonia, assuming constant temperature and pressure?
• How would you calculate the mass in grams of hydrogen chloride produced when 4.9 L of molecular hydrogen at STP reacts with an excess of chlorine gas.?
• Question #a6256
• What mass of calcium when reacted with water will produce 15.7 L of hydrogen at STP?
• Given the equation: #N_2 + 3H_2 -> 2NH_3# What volume of hydrogen is necessary to react with five liters of nitrogen to produce ammonia? (Assume constant temperature and pressure)
• Question #91883
• How many moles of #H_2# are needed to react with .80 mol of #N_2#?
• What volume of #O_2# at 912 mmHg and 21° C is required to synthesize 18.0 mol of #NO#?
• A #30*L# volume of dioxygen gas at #473*K#, and a pressure of #2*atm#, will completely combust WHAT mass of #"ethane gas"#?
• How many liters of O2 (g) are needed to react completely with 56.0 L of CH4 (g) at STP to produce CO2 (g) and H2O (g)? Given: CH4 (g) + 2O2 (g) → CO2 (g) + H2O (g)
• If 1 mol #N_2#(g) reacts with 3 mol #H_2# (g) in a flexible container at constant temperature and pressure, would you expect the total gas volume to increase or decrease?
• How many liters of oxygen would be needed to produce 45.0 liters of carbon dioxide if the temperature and pressure for both are 22.0° C and 75.0 psi?
• What is the volume of #NH_3# produced in the following reaction when 3.0 L of #N_2# reacts with 4.0 L of #H_2#?
• Question #67fff
• How many moles of gas at 5.60 atm and 300 K will occupy a volume of 10.0 L?
• Assuming all volume measurements are made at the same temperature and pressure, what volume of hydrogen gas is needed to react completely with 4.55 L of oxygen gas to produce water vapor?
• Propane, #C_3H_8#, reacts with oxygen to produce carbon dioxide and water. If 10.0 grams of oxygen reacts with an excess of propane, then how many moles of carbon dioxide were produced?
• Question #0c07e
• If a sample of 4 moles of gas has a pressure of 567.42 kPa and a volume of 12.0 L, what is its temperature?
• How many mL of carbon tetrachloride are produced when 8.0 L of chlorine are allowed to react with 0.75 L of methane at STP?
• If iron (II) oxide gas decomposes into iron liquid and oxygen gas and 6 moles of iron (II) oxide gas are used, how of liters of oxygen gas are produced?
• An ideal gas is compressed at a constant pressure of 120 kPa to one-half of its initial volume. The work done on the gas is 790 J. What was the initial volume of the gas?
• A gas occupies 12.3 L at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 60.0 mm Hg?
• What volume of ammonia, in #cm^3#, can be prepared by reacting 20 #cm^3# of nitrogen gas with 30 #cm^3# of hydrogen gas?
• 10 #cm^3# of carbon monoxide and 10 #cm^3# of oxygen are mixed. What will be the total volume of gas present, in #cm^3#, after the reaction?
• What volume of #"NH"_3# at STP is produced if #25.0 "g"# of #"N"_2# is reacted with an excess of #"H"_2# in the reaction #"N"_2 + 3"H"_2 -> 2"NH"_3#?
• In the reaction #NH_4NO_2(s) -> N_2(g) + 2H_2O(g)#, how many liters of nitrogen gas is produced if 50.0 L of water is produced at STP?
• How many liters of carbon dioxide are produced when 2.0 moles of #CH_4# are burned at #STP#?
• How many liters of nitrogen monoxide will be obtained from 2.50 liters of oxygen if the temperature and pressure are constant?
• What volume of oxygen is needed to completely combust 2.36 L of methane gas #CH_4#?
• Question #8d65b
• How many grams of Na(l) are produced per litre of N2(g) formed in the decomposition of sodium azide, NaN3 if the gas is collected at 25 degrees celsius and 1.0 bar (.98692 atm)? The R constant is 0.08206 Latm/Kmol
• How many moles of oxygen gas are required to combust a #4*mol# quantity of acetylene completely?
• In methane combustion, if #2.5*mol# #O_2# were present, what molar quantity of methane would react?
• How should liquid nitrogen and liquid oxygen be stored and dispensed? What safety equipment and precautions are employed?
• How many grams of lithium metal are required to react with a #28*g# mass of dinitrogen gas?
• What is #[HCl(aq)]# in the following scenario?
• Question #11cbb
• What is the concentration of #1.12*L# of carbon dioxide gas?
• Ammonia is produced in the reaction #3H_2 + N_2 -> 2NH_3#. What mass of #NH_3# could be produced if 12.5 #H_2# reacts with excess nitrogen?
• How many liters of oxygen gas are produced by the complete decomposition of 225 mL of water?
• If 538 mol of octane combusts, what volume of carbon dioxide is produced at 14.0°C and .995 atm?
• When 2.5 liters of oxygen gas reacts with excess methane how many liters of carbon dioxide is produced?
• In the formation of carbon dioxide from carbon monoxide and oxygen, how many liters of carbon monoxide, CO, are needed to react completely with 1/2 mole of oxygen gas at STP? 2 CO (g) + O2(g) → 2 CO2 (g)
• Question #e7ecb
• An excess of hydrogen reacts with 14.0 g of #N_2#. What volume of ammonia will be produced at STP?
• Question #fcb1b
• Question #dfbe7
• Question #ca67b
• How many grams of #CO_2# and grams of #H_2O# are produced when 52.0 g #C_2H_2# burns in oxygen?
• What volume of oxygen gas is needed to completely combust 0.202 L of butane gas?
• What volume of ammonia gas, NH3, in liters is produced at stp by the complete reaction of 100 g of nitrogen N2, with excess hydrogen? N2 + 3H2 ---> 2NH3
• What volume of oxygen is needed to react with solid sulfur to form 6.20 L of sulfur dioxide?
• How many mols of oxygen are required to react completely with 81 L of hydrogen to form water?
• How many liters of oxygen are required to react completely with 1.2 liters of hydrogen to form water?
• How would you find a balanced equation if acetylene gas (#"C"_2"H"_2#) undergoes combustion to form carbon dioxide and water vapor?
• How many grams of ammonia, #NH_3#, would be formed from the complete reaction of 4.50 moles hydrogen, #H_2# in the reaction #N_2 + 3H_2 -> 2NH_3#?
• How many liters of carbon dioxide can be produced if 37.8 grams of carbon disulfide react with excess oxygen gas at 28.85 degrees Celsius and 1.02 atmospheres?
• How many moles of ethylene (#C_2H_4#) can react with 12.9 liters of oxygen gas at 1.2 atmospheres and 297 Kelvin?
• Ammonia gas decomposes according to the equation: #2NH_3(g) -> N_2(g) + 3H_2(g)#. If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)?
• Methane reacts with steam to form #"H"_2# and #"CO"# as shown. What volume of #"H"_2# can be obtained from #"100 cm"^3# of methane at STP?
• Question #39c68
• Question #05592
• Question #5b125
• Question #928a6
• Given the following, how many grams of water could be produced in this reaction? What is the limiting reactant? If 8.7 g of water are produced, what is the percent yield?
• Question #a2839
• Question #11371
• #H_2(g) + Cl_2(g) rarr 2HCl(g)# The give reaction occurs at constant pressure...which is the only viable observation?
• A #15*g# mass of methane is combusted with a #50*g# mass of dioxygen gas. Will combustion be complete?
• Question #fd292
• How many liters of #O_2# gas, measured at 777 mm Hg and 35°C, are required to completely react with 2.7 mol of #Al#?
• A #30*L# volume of dinitrogen reacts quantitatively with a #60*L# dihydrogen to give ammonia. What volume of ammonia results under the same conditions, and what is the volume of the excess reagent?
• Question #934b0
• Question #ad087
• What is #"NTP"#?
• Ammonia gas is synthesized according to the balanced equation below. N2 (g) + 3 H2 (g) → 2 NH3 (g) If 2.75 L N2 react with 7.75 L H2, what is the theoretical yield (in liters) of NH3?
• Question #8ebae
• Question #4cfd2
• If a #34.7*L# quantity of dihydrogen gas reacts with stoichiometric #Cl_2#, what VOLUME of #HCl(g)# will result under standard conditions?
• Question #94034
• Question #25d7e
• Question #fae95
• Question #3fb7d
• What volume of ammonia is produced by the reaction when #"19.5 L"# of hydrogen gas react at #93^@"C"# and #"48.7 kPa"# ?
• Question #69942
• Question #c5367
• Under standard conditions, what volume does a #25*g# mass of ammonia gas occupy?
• Question #ee172
• When calcium carbonate is decomposed, what mass of carbon dioxide is evolved?
• How do you find the mass of sodium required to produce 5.68 L of hydrogen gas STP from the reaction described by the following equation: #2Na + 2H_2O -> 2NaOH + H_2#?
• Question #c6f97
• Question #1de47
• Question #296b3
• What volume of dihydrogen gas will be generated by the action of excess hydrochloric acid on a #21*g# mass of zinc metal?
• How many moles of hydrogen gas can be evolved from the action of excess hydrochloric acid on a mass of #4.8*g# of magnesium metal?
• Question #b6a10
• What are the volumes of each gas in the resulting mixture after the combustion of #"20 cm"^3 color(white)(l)"CO"# with #"30 cm"^3color(white)(l)"O"_2#?
• How many grams of CO2 would be produced if 350.0 mL of diethyl ether were combusted in an unlimited amount of oxygen ? Density of diethyl ether is 0.713g/mL. C4H10O + O2 ---> H2O + CO2 Thanks for all your content!
• If #12*L# of hydrogen gas react with #12*L# of chlorine gas, what volume of #HCl(g)# will result?
• Propane is combusted completely in air. What volume of dioxygen gas is required to combust a #200*mL# volume of propane?
• Question #1199a
• What mass of carbon dioxide results from complete combustion of a #9.75*L# volume of benzene?
• A volume of #20*cm^3# acetylene was combusted with a volume of #500*cm^3# dioxygen in a piston. What is the end volume of the gases confined by the piston?
• How many moles of propane gas (#"C"_3"H"_8#) can be burned with 1 mole of oxygen gas at STP?
• What volume of propane consumes one litre of oxygen during its complete combustion?
• 0.25 pts What is the total number of molecules in 11.2 liters of #N_2# gas at STP?
• If #100*mL# of ammonia gas are decomposed into its constituent elements what volumes of dinitrogen, and dihydrogen would result?
• For the combustion reaction #4"NH"_3(g) + 5"O"_2(g) -> 4"NO"(g) + 6"H"_2"O"(g)#, how many liters of #"O"_2(g)# would react with #"500 L"# of #"NH"_3# at STP?
• (8.000x10^-1) g of a gas is collected in the lab and found to have a volume of (8.9000x10^-1) L when the pressure is (9.600x10^1) kPa and the temperature is (3.00x10^2) K. According to this collected data what is the molar mass of the gas?
• Question #4187f
• What volume of water results from complete combustion of a #40*L# volume of methane under standard conditions?
• A 2.0 liter container of nitrogen had a pressure of 3.2 kPa. What volume would be necessary to decrease the pressure to 1.0 kPa?
• Air is approximately 79% nitrogen and 21% oxygen by volume. How many moles of oxygen are present in 22.0 L of 24 C and a pressure of 53 kPa?
• Question #ae352
• If 2.54 L of hydrogen reacts with 3.13 L of oxygen at temperatures above 100 degrees Celsius, how many L of H2O(g) will form?
• Magnesium will burn in oxygen to form magnesium oxide as represented by the following equation 2Mg(s) + O2(g) -> 2MgO(s) What mass of magnesium will react with 498.1 ml of oxygen at 145.2 degrees Celsius and 0.927 atm?
• How many liters of hydrogen gas can be produced at 313.4 K and 105.3 kPa if 23.4 g of sodium metal is completely reacted with water according to the following equation? 2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g)
• Question #74040
• How much octane could a #0.500*L# volume of air completely combust?
• Question #12a91
• Question #2494a
• What volume of carbon dioxide gas will result from the complete combustion of a #2500*L# volume of propane?
• Under conditions of #"NTP"#, what volume of #SO_2(g)# results from burning a #10*g# mass of elemental sulfur?
• What mass of sodium chloride, #NaCl#, is made when #200# #L# of chlorine gas, #Cl_2#, reacts with excess sodium metal?
• For the reaction #CH_4 + 2O_2 -> CO_2 + H_2O#, how many moles of carbon dioxide are produced from the combustion of 100. g of methane?
• Question #6922c
• Ethene undergoes incomplete combustion to form carbon dioxide, carbon monoxide and water vapour. If the ratio of carbon dioxide to carbon monoxide formed is 9:1 when x cm^3 of ethene is burnt, what is the volume of oxygen gas consumed in the reaction?
• Question #a9d2d
• Question #a55bf
• The number of litres of air required to burn 8 litres of C2H2 is approximately?
• Question #0fbb3
• Question #b584a
• #15cm^3# of a mixture of ethane and methane were completely oxidized by #43cm^3# of oxygen. The volumes were measured at the same temperature and pressure. What was the composition of the mixture?
• Question #e1092
• Question #42d80
• Given EXCESS zinc metal, what volume of dihydrogen gas at #"NTP"# will be evolved from the action of #500*cm^3# of #H_2SO_4# at #0.50*mol*L^-1# concentration?
• Question #df311
• Ammonia reacts with oxygen according to the equation given below. If a #"72.0-mL"# sample of #"NH"_3# gas is allowed to react with excess oxygen at room temperature, #25^@"C"#, and #"1 atm"#, calculate the number of molecules of water produced?
• How do we represent the reduction of #100*L# of #"potassium chlorate"#?
• Question #67c37
• What mass of calcium carbide, #Ca^(2+)C-=C^(2-)# will give a #1.12*L# volume of acetylene gas upon treatment with water?
• Question #e4d8f
• Question #6be2c
• Question #71e84
• The flame produced by the burner of a gas (propane) grill is a blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely?
• How many grams of sodium azide are needed to provide sufficient nitrogen gas to fill a 50.0 × 50.0 × 25.0 cm bag to a pressure of 1.15 atm at 25.0 °C? 
• A #30*L# volume of carbon monoxide is reacted with a #10*L# volume of oxygen gas. How much carbon monoxide remains unreacted?
• How much carbon dioxide is exhaled if an animal inhales 32.0 g #O_2#?
• Question #6f9c1
• Question #8c2bd
• Question #e1374
• Can we use fractional coefficients in stoichiometric equations?
• #"1 L"# of #"CO"_2# is passed through red hot coke. The volume becomes #"1.4 L"# at the same temperature and pressure. What is the composition of the products?
• A #600*cm^3# volume of ethane gas is completely combusted with #2500*cm^3# of dioxygen gas to give carbon dioxide and water. What is the reagent in excess, and what volume would #CO_2(g)# occupy after the reaction....?
• 20 mL of methane is completely burnt using 50 mL of oxygen. The volume of the gas left after cooling to room temperature is? A) 80 B)40 C) 60 D) 30
• If a #10*mL# volume of nitrogen gas reacts with stoichiometric hydrogen, what is the likely volume of ammonia gas produced?
• What volume of nitrogen monoxide is produced when #"146 L"# of ammonia react according to the following reaction? (All gases are at the same temperature and pressure.)
• Determine how many liters of nitrogen will be required to produce 214.4 liters of ammonia? The balanced equation for this reaction is: #3"H"_2(g) + "N"_2(g) -> 2"NH"_3(g)# ?
• A liter of air containing 1% Ar is repeatedly passed over hot Cu and hot Mg till no reduction of volume takes place. The final volume of Ar will be?