How many grams of NaOH are needed to produce 5.00 L of H2 gas at 285K and a pressure of 99.9 kPa? 2 As + 6 NaOH → 2 Na3AsO3 + 3 H2 21.3 g 85.2 g 0.211 g O 16.9 g

Q: Ammonium carbonate decomposes upon heating according to the balanced equation:(NH4)2CO3(s)----->…

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Q: What is the volume of a gas if 1.75 moles of the gas has a pressure of 315 kPa at 273K? 12.6 liters…

A: Given the number of moles of gas =1.75 molpressure of gas =315 kPa =3.10881 atm   ( 1atm =101.325…

Q: What is the pressure, in kPa, exerted by 5.5 moles of O2 in a 50.0L container at 30.0°C? ОА. 325 kРа…

A: Use Ideal gas law to find out the pressure exerted by the gas,PV = nRTGiven that, number of moles, n…

Q: How many grams of NaN 3 would be required to provide 75.0 L of N 2 gas at 25°C and 748 mmHg? 6NaN 3…

A: The balanced reaction is: Calculation of no. of mol of N2 gas: According to the ideal gas equation,…

Q: is the molar mass of a gas that has a sample mass of 3.17 g and occupies a volume of 548 mL at 2.00…

A: Answer  Calculate molar mass of gas   Gas equation   PV   =    nRT…

Q: If a gaseous mixture is made by combining 4.77 g Ar and 2.34 g Kr in an evacuated 2.50 L container…

A: Pi = Xi x P Where, Pi = partial pressure of gas i,             Xi = mole fraction of gas i…

Q: Acetylenee gas can be produced by slowly reacting Calcium carbide with water. CaC2 (s) + 2H2O (l) →…

A: CaC2+2H2O→C2H2 +CaOH2moles of CaC2=mass molar mass=4564=0.70According to equation ,1 mol CaC2 form…

Q: 6. Calculate the total pressure of a mixture that contains 1.00 g H2 and 1.00 g of He in a 5.00 L…

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Q: A gas mixture contains O2, N2, and Ar at partial pressures of 125, 175, and 225 mm Hg, respectively.…

A: Given details, At partial pressures, P(O2)=125 mm HgP(N2)=175 mm HgP(Ar)=225 mm Hg Then, the total…

Q: What is the density in grama per 1iter of neon gas at 3.00 kPa and 20.0°C in a 2.00 L container?…

A: P = 3kPa = 0.0296 atm  T = 20oC = 293.15K V = 2L R = 0.082Latmmol-1K-1

Q: What volume of gas is produced when 16.0 g of lithium reacts with 30.0 mL of water? Assume that the…

A: Given, Mass of Li  = 16.0 g  Volume of water = 30.0 mL  Density of water = 1.00 g/mL  Pressure =…

Q: A 1.00 L sample of dry gas at 16 °C and 744 mmHg contains 0.520 g N₂. What is the partial pressure…

A: Given that, Volume of the dry gas is 1.00 L. Temperature = 160C Total pressure = 744 mm Hg Mass of…

Q: What volume of gas is produced when 16.0 g of lithium reacts with 30.0 mL of water? Assume that…

A: The reaction is as follows; 2Lis+2H2Oaq→2LiOHaq+H2g 1 mol of H2O reacts with 1 mol of Li 18 g of H2O…

Q: 7) The density of Cl2gas at STP, in grams per liter, is approximately: (а) 1.3 (b) 3.9 (c) 4.5 (d)…

A: d) 3.2 We know that,  Molar mass of Cl2 gas = 70.906 g Volume of 1 mole of Cl2 gas at STP = 22.4 L

Q: What is the molar volume of an ideal gas at 546 R and 1.00 atm? 16.9 L 89.6 L 22.4 L 11.2 L 44.8 L

A: To calculate the molar volume of an ideal gas at 546 K and 1.00 atm.

Q: What volume of oxygen gas is produced when 29.4 g of mercury(II) oxide reacts completely according…

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Q: Please show solving steps

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Q: What volume of gas is produced when 16.0 g of lithium reacts with 30.0 mL of water? Assume that…

A: Lithium reacts with water to produce lithium hydroxide and hydrogen gas. Reaction can be represented…

Q: A flask contains 1000 ml of a pure diatomic gas 646 mm Hg and 20 degrees mass of gas is 1.13 g. What…

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Q: What is the total volume of gases produced at 1092 K and 1.20 atm pressure when 320 g of ammonium…

A: Answer = d. 1121 L

Q: A sample of nitrogen occupies 945 mL at a temperature of 26 °C and a pressure of 85.0 kPa. What…

A: PV = nRT Volume of gas at STP = n x 22.4 L

Q: If you have 10 L. Hydrogen gas at 101.3 kPa. What will the new volume be if the pressure increases…

A: The question is about calculating the new Volume when the pressure increases to 405.2 kPa -

Q: An empty 2.10-L vessel weighs 92.00 g. After filling the vessel with 1.00 atm of a gas at 27.0 °C,…

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Q: What is the minimum volume, in mL, of 6.0 M H3PO4 necessary to produce 43.6 L of H2 gas in the…

A: First, calculate the number of moles of H2 gas using the ideal gas equation: PV =…

Q: What volume of chlorine gas at 20.0°C and 95.5 kPa is needed to produce 65.0g of HCI? H2 + Cl2 2HCI…

A: Given the chemical reaction as follows,H2+Cl2→2HClwe are to calculate the volume of chlorine gas at…

Q: Consider the generic reaction: 2 A(g) + B(g)》2 C(g). If a flask initially contains 1.0 atm of A and…

A: Reaction proceeds to completion implies that almost all of the reactants are converted into product.…

Q: A 1.95 g sample of an unknown gas at 61 ∘C and 1.00 atm is stored in a 1.45 L flask. What is the…

A: Given information:Mass of sample = 1.95 gTemperature = 61 °CPressure of gas = 1.00 atmVolume of…

Q: For the reaction: N2(g) + 3Hz(g) =2NH3(g)  what is the volume (L) of H2 gas needed to produce 4.00g…

A: Reaction equation :N2(g) + 3H2(g) ⇌                 2NH3(g)Mass of ammonia = 4.00 gramsTemperature =…

Q: Sodium hydroxide reacts with aluminium powder according to the following reaction:   2 NaOH(aq) +…

A: Given reaction; 2 NaOH(aq) + 2 Al(s) + 6H2O(l) → 2 NaAl(OH)4(aq) + 3 H2 (g) Given amount of Al = 5.2…

Q: What volume (L) of NH3 gas at 1.2182 atm and 298 K is produced by the complete reaction of 19.32 g…

A: Given: Pressure = 1.2182 atm  Temperature = 298K  Mass = 19.32 g  To find : Volume of NH3 in liters…

Q: Calculate the mass of 6.2 L of CO2 at 300° K and a pressure of 758.0 mm Hg.

A: CO2 gas Volume = V = 6.2 L Temperature = T = 300 K Pressure = P = 758.0 mm Hg ( 1 atm = 760 mm Hg )…

Q: If a gaseous mixture is made by combining 1.29 g Ar and 2.46 g Kr in an evacuated 2.50 L container…

A: The total pressure of a mixture of two non reacting gases is given by  PtotalV = (n1+n2)RT  Ptotal =…

Q: What volume would 15.2 g of a gaseous compound occupy at STP if its molecular weight is 44.0 g/mole…

A: Concept is based on ideal gas:

Q: What is the mole fraction of NO in a 55.0-L gas cylinder at 30°C which comes from a mixture of N2…

A: Gases that comprises of zero particle interaction and additionally, particles possess elastic…

Q: 10) Iron nail rusts when exposed to oxygen.4Fe(s) + 3 O2(g)2 Fe2O3(s) a)What volume of oxygen gasat…

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Q: Two gas bulbs are connected by a thin tube. Calculate the partial pressure of Argon (in atm) after…

A: To calculate the partial pressure of argon , we would use Boyle's law, because the gases are mixed…

Q: What is the mass (in grams) of an unknown gas (molecular weight = 295 g/mol) that is contained in a…

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Q: How many grams of Chlorine gas are needed to occupy a 10.0 liter gas cylinder with a pressure of…

A: Ideal gas equation :-  PV = nRT  P= pressure  V= volume  n = no. of moles  R = gas constant  T =…

Q: Constants R = 0.0821atmolmolK . 1atm = 760mmHs , 1 gas = 22.41 (STP)  Hydrogen was prepared in 1776…

A: Since from the given reaction we can say that 3 moles of Fe is reacting to form 4 moles of H2  Hence…

Q: A 1.95 g sample of an unknown gas at 67 °C and 1.05 atm is stored in a 2.05 L flask. What is the…

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Q: What is the total pressure exerted by a mixture of 2.00 g ofH21g2 and 8.00 g of N21g2 at 273 K in a…

A: The given data contains, Volume = 10.0 L. Temperature =273 K gas constant R =0.0821 L.atm.mol-1K-1

Q: 0.374 m3 of hydrogen was observed at −7.0 oC and atmospheric pressure (105 Pa). The relative…

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Q: What is the total volume of gases produced at 1092 K and 1.00 atm pressure when 320 g of ammonium…

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Q: 10. Consider the formation of nitrogen dioxide from nitric oxide and oxygen: 2NO(g) + 02(g) -->…

A: PV = nRT  This is ideal gas equation. At constant temperature and pressure condition  number of…

Q: What is the mole fraction of N2 if a flask contains a mixture of 1.11 g H2 gas (H = 1.01 g/mol) and…

A: Mole fraction is defined as number of moles of solute divided by total number of moles of solution.…

Q: 4 C3H5N3O9(l) + 6 N2(g) -> 12 CO2(g) + 10 H2O(g) + 1 O2(g) a. If 2.00 x 102 g worth of…

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Q: How many grams of H2O are needed to produce 50.0 L of NH3 gas at 298K and a pressure of 175 kPa?…

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Q: A sample of CO2 gas occupies a volume of 250 mL at 100 °C and 450 mm Hg pressure. What will be its…

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Q: A 4.00 L flask filled with He at 6.00 atm is connected to another 2.00 L flask containing N2 at 3.00…

A: Considered that the temperature of the system is 298.15 K. The number of moles of He and N2 is…

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.