In the scenario above, if 6.54 g of sodium hydrogen carbonate is combined with a slight excess of acetic acid solution, how much carbon dioxide, in mL, would be produced?

Q: If a gaseous mixture is made by combining 2.15 g Ar and 3.13 g Kr in an evacuated 2.50 L container…

A:

Q: A certain gas sample has a volume of 225 mL at a pressure of 1.25 atm at 27oC; what would be its…

A: Given: P1 = 1.25 atm V1 = 225 ml P2 = 0.75 atm V2 = ? according to boyles at constant temperature.…

Q: A mixture of gases contains 2.08 g of CO, 4.02 g of Xe, and 7.90 g of N2O. What is the partial…

A: option c correct From the Ideal Gas Lawp × V = n× R × Tn = mMp=m× R× TM ×Vwhere p= pressurem=massM=…

Q: Consider the balanced reaction below: AB(s) + 2 DE (aq) → 3 R2 (g) + 4 Q (aq) When the reaction…

A: When a gas is collected over water, some water vapours also present along with the gas. The pressure…

Q: 13. Some 02(g) was collected over water in a volume of 55.3 mL at 20. °C under atmospheric pressure…

A: Consider the given information is as follows; Volume of water (V) = 55.3 mL = 0.0553 L Temperature…

Q: A gas cylinder contains 2.2 mol of N2, 3.3 mol of O2 and 4.4 mol of Cl2. What is the partial…

A: The partial pressure (Pa) of a gas 'a' in a mixture is given by: Pa=χa×PT Here PT is the total…

Q: Consider the following decomposition of sulfurous acid, H₂SO3: H₂SO3(aq) → H₂O(l) + SO₂(g). How many…

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Q: At 2°C a 1.0-L flask contains 1.0x 10^-2  mole of N2 , 4.0x10^2 mg O2 , and 5.1x 10^21 molecules of…

A: N2 =  1.0x 10^-2  mole = 0.01 mole O2 =  4.0x10^2 mg =400 mg =0.4 g O2 = 0.4 g / 32g/mol = 0.0125…

Q: SO2 (0.0780mol) and CO2 (0.114mol) are placed in a 750.mL container at 50.0˚C. What is the partial…

A: Ideal gas equation is: PV = nRT…

Q: consider an experiment where 4.55mL of an unknown H2O2(aq) solution reacted with the yeast at 19.1 C…

A: Given , Partial pressure of O2 gas collected = 1.0126 atm moles of O2 produced = 0.004142 mol

Q: A mixture of HeHe, ArAr, and XeXe has a total pressure of 2.90 atmatm . The partial pressure of HeHe…

A: If a vessel is filled with more than one gas then the each gas exerts the pressure. The pressure of…

Q: sealed container is filled with 3.00 g of CO2 (MM = 44.01 g/mol), 5.00 g of Kr (MM = 83.80 g/mol),…

A:

Q: A certain laser uses a gas mixture made of 1.00 g hydrogen gas, 4.50 g hydrogen chloride, and 82.5 g…

A: Concentration of the solution can also expressed by mole fraction. Mole fraction is equal to moles…

Q: A neon sign is made of glass tubing whose inside diameter is 2.0 cm and whose length is 4.0 m. If…

A: P = 1.5 mm Hg T = 350C = 308 K Radius = 1 cm = 0.01 m Length = 4 m

Q: A mixture of 17.9 g N2 (Molar mass: 28.0 g/mol), 36.9 g Cl2 (Molar mass: 70.9 g/mol) and 18.4 g Xe…

A: The given problem can be solved by using the formula given below as;…

Q: The following reaction yields 28.4 g of CH3OH: CO(g) + 2 H2(g) --> CH3OH The molar mass of CH3OH is…

A: The given reaction is as follows-      CO(g) + 2H2(g) ---> CH3OH yield of CH3OH = 28.4 g  We have…

Q: A mixture containing 2.13 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a…

A: To solve this problem we will use Ideal gas equation  PV = nRT  Where , P = pressure…

Q: A different tank of gas contains 2.0 mol of oxygen gas (02) and 2.0 mol of hydrogen gas (H2) at a…

A: Answer:When volume and temperature of the system is constant then pressure is directly proportional…

Q: Suppose 2.80% of 480 g of PCls (208.2 g/mol) initially present in a 7.00 L reaction vessel at 300°C…

A:

Q: A 2.01 L flask containing 2.31 g of helium gas (molar mass = 4.003 g/mol) is separated by a stopcock…

A: Solution:      Number of moles in a solution is given by the ratio of number of moles of substance…

Q: Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g) +3 F2(g) → 2 CIF 3(g) If…

A: The balanced chemical equation is as follows:The volume of chlorine gas = The volume of fluorine gas…

Q: The temperature in the room is 21 oC and the pressure is 638 torr.   1 atm = 760 torr and R =…

A: Given, Temperature = 21 oC                      = 294 K P = 638 torr    = 0.8395 atm R = 0.08206 L…

Q: Please don't provide handwritten solution ....

A: The objective of the question is to find out the volume of Cl2 required to react with 3.6 L of NO2…

Q: Hydrogen was collected over water at 21.4°C on a day when the atmospheric pressure was 741 Torr. the…

A:

Q: 73. Oxygen gas, generated by the reaction 2KCI03(s) → 2KCI(s) + 3O2(g), is collected over water at…

A:

Q: At 22°C and 0.998 atm, what is the theoretical volume (in mL) of hydrogen gas produced when 0.45g of…

A:

Q: Acetylene is manufacture by hydrogenation of C (graphite): 2 C (s) + H₂ (g) → C₂H₂ (9) How much kg…

A:

Q: A gaseous "CFC" compound has a density of 5.456 g/L at 0.993 atm and 22.0°C. (a) Calculate the molar…

A: Given , density of CFC =5.456gL Pressure = 0.993 atm temperature, T=22°C =(22+273)K=295 K

Q: Consider 100.0 mL samples of O2 (g), N₂ (g), and Cl₂ (g) at the same temperature. Which of the…

A: 100.0 mL samples of O2 (g), N2 (g), and Cl2 (g) at the same temperature.

Q: A mixture of gases contains 3.46 g of SO2, 5.53 g of H2, and 1.50 g of O2. What is the partial…

A:

Q: Given the reaction: 2 Na (s) + H₂SO₄ (aq) → Na₂SO₄ (aq) + H₂ (g) What volume of H₂ (in liters) could…

A: The stoichiometric relation in the given balanced chemical equation is  moles of H2…

Q: A chemistry student places 5.35 grams of aluminum metal into phosphoric acid.  The reaction gives…

A: Given: The mass of aluminium metal taken = 5.35 grams The percent yield = 78.5% We have to calculate…

Q: Using the procedure in Experiment 8, acetonitrile (molar mass = 41.05 g/mol) is collected at a…

A: Answer:- This question is answered by using the simple concept of calculation of volume of a gas…

Q: Please don't provide handwritten solution ...

A: The objective of the question is to determine the limiting reactant, the theoretical yield in moles,…

Q: Consider the following gas phase reaction. 4HCl(g) + O2(g) -> 2Cl2(g) + 2H2O(g) What mass of…

A: We have to calculate the mass of Cl2 produced from 400 ml of HCl measured at STP.

Q: A mixture containing 2.21 g each of CH4(g), C,Ha(g) and CaH,o(g) is contained in a 1.50 L flask at a…

A:

Q: What volume (L) of H2 gas is produced when 92 g Zn (atomic weight: 65.38 g/mol) is decomposed…

A: Given: The mass of zinc is 92 g and its molar mass is 65.38 g/mol. The temperature is 0°C and…

Q: Magnesium metal reacts with hydrochloric acid to producing hydrogen gas according to the following…

A: Given,

Q: 11. What volume of hydrogen gas at STP may be prepared by the reaction of 4.54 g of gallium with…

A: Given, Ga(s) + HCl(aq) ➝ GaCl3 + H2 Mass of Ga reacts = 4.54 g Molarity of HCl solution = 1.75 M =…

Q: A sample of a smokestack emission was collected into a 1.10-L tank at 742 mm Hg and analyzed. The…

A: In 100 g sample mass of CO2= 92 g  Mass of NO = 4.2 g  Mass of SO2 =1.3g Mass of H2O = 2.5g  Molar…

Q: Consider the following reaction for the combustion of octane, C8H18: 2 C8H18(l) + 25 O2(g) → 16…

A:

Q: The temperature difference between day and night on Mars is much bigger than on Earth, due to its…

A: Given: The initial temperature, (T1) =  21 oC = (273.15 + 21) = 294.15 K. The final temperature,…

Q: Q5. A 31.3 mL sample of an unknown, water-insoluble gas was collected over water at 20.4°C and a…

A: Given data,Volume of sample=31.3mL=0.0313LTemperature=20.4oC=20.4+273=293.4KBarometric…

Q: A mixture of gases contains 3.16 g of 03, 7.86 g of H2, and 2.79 g of SF6. What is the partial…

A: Partial pressure of a gas is its pressure in a mixture of gases. The pressure of each gas can be…

Q: The combustion of fuel in your car engine requires oxygen gas, which is supplied as air (21% oxygen…

A: Given data : Volume of air = 2.71 L          Pressure = 1 atm          Temperature = 25°C = 298 K…

Q: Find the pressure in Torr of 0.0080 mol of an ideal gas contained in 125 L at 15 °C: R = 62.36…

A: The ideal gas equation is  PV = nRT  P = pressure  V = volume  n = moles of gas R = gas constant =…

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.