If 9.86 L of gaseous Cl2 measured at STP and 63.2 g of liquid CS2 are reacted stoichiometrically according to the balanced equation, how many milliliters of liquid CCl4 are produced? CS2(l) + 3Cl2(g) → CCl4(l) + S2Cl2(l) Molar Mass (g/mol) Cl2 70.906 CS2 76.143 CCl4 153.82 Density (g/mL)     CS2 1.26 CCl4 1.60 Molar Volume (L) 22.4 at STP Gas Constant(L.atm.mol-1.K-1) 0.0821

Q: A gaseous mixture of N2 and O2 has a total pressure of 1.760 atm. If the partial pressure of N2 is…

A: Given, Total Pressure= 1.760 atm Partial pressure of N2 = 0.682 atm

Q: If 56.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

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Q: If 72.6 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A: The reaction taking place is given as, => H2CO3 (aq) ----> H2O (l) + CO2 (g) Given : Volume of…

Q: Calculate the volume of methane, CH4 , at STP required to completely consume 3.5 L of oxygen at STP

A: Given, Volume of O2 = 3.5 L  Volume of methane = ?

Q: If 60.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

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Q: At 7°C a 1.0-L flask contains 5.0 × 10-2 mole of N2, 2.0 x 102 mg 02, and 2.4 x 1021 molecules of…

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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),…

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Q: moles

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Q: A mixture of carbon dioxide and argon gases contains carbon dioxide at a partial pressure of 278 mm…

A: Since we know that the mole fraction of any gaseous system is also equal to the partial pressure…

Q: A gaseous compound has a density of 1.87 g/L at 22.0 °C and 1.41 atm. What is the molar mass of the…

A: Given  , Density  of gas = 1.87 g/L Pressure  of gas= 1.41 atm Temperature  of gas =  22.0°C =( 22+…

Q: A gaseous compound has a density of 1.12 g/L at 23.3 °C and 1.11 atm. What is the molar mass of the…

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Q: How many grams of CaCO3 (100.09 g/mol) would be needed to produce 34.5 L of CO2 at STP?…

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Q: Consider the following balanced equation. 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) What volume of…

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Q: Assume a gas mixture consists of 0.215kg of Xe, 258g of H2, 51.8g of Cl2, and 283g of C6H6. If the…

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Q: Determine the mass of water formed when 12.5 L NH3 (at 298 K and 1.50 atm) is reacted with 18.9 L of…

A: The balanced reaction taking place is given as, => 4 NH3 (g) + 5 O2 (g) -----> 4 NO (g) + 6…

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: A mixture of neon and methane gases contains neon at a partial pressure of 406 mm Hg and methane at…

A: Relation between Mole fraction and Partial pressure:  χA = nAnT = PAPT

Q: Oxygen gas can be prepared by heating potassium chlorate according to the following equation:…

A: The partial pressure of O2, PO2, and the number of moles of O2 is calculated as shown below.…

Q: Potassium reacts with water to release hydrogen gas according to the following equation: 2 K (s) + 2…

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Q: A gaseous compound has a density of 1.69 g/L at 25.2 °C and 1.45 atm. What is the molar mass of the…

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Q: Two bulbs are separated by a valve. Bulb A contains 1.2 L He gas at 0.63 atm and 16°C. Bulb B…

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

Q: What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's…

A: Volume can be converted to mass using density. The equation is; density=massvolume Ideal gas…

Q: A mixture contains 5.00 g each of O2, N2, CO2, and Negas. Calculate the volume of this mixture at…

A: Given : Gaseous mixture contains O2, N2, CO2 and Ne gas. And mass of each gas is 5.00 g.

Q: If 67.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

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Q: if 90.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298 K) and…

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Q: A gaseous compound has a density of 1.36 g/L at 23.5 °C and 1.50 atm. What is the molar mass of the…

A: Given Density = 1.36 g/L Temperature = 23.5 oC = ( 273 + 23.5 ) = 296.5 K Pressure = 1.50 atm

Q: A student recovered0.398g of THF vapor in a 125 mL flask. Assuming the vapor is an ideal gas with a…

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Q: How many liters of CH₃OH gas are formed when 3.20 L of H₂ gas are completely reacted at STP

A: Given, volume of H2 = 3.20 L  One mole of gas occupies 22.4 L  We First find Number of moles of…

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

A: It is given to us that the ethanol is used 100% in the reaction and the volume of oxygen-1.92 L at a…

Q: How many grams of Na solid are required to completely react with 19.2 L of Cl₂ gas at STP according…

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Q: CO2 was added to a cylinder containing 2.5 atm of O2 to give a total pressure of 4.0 atm of gas.…

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Q: A gaseous compound has a density of 1.67 g/L at 22.1 °C and 1.42 atm. What is the molar mass of the…

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Q: A gaseous compound has a density of 1.64 g/L at 21.6 °C and 1.27 atm. What is the molar mass of the…

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Q: What is the mass (in grams) of 25.00 L of propane vapor (C³H³) at STP? R=0.08314 L-bar/mol.K.

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Q: A mixture of the gases N2, O2, and He has a total pressure of 760 mm Hg. If the partial pressure of…

A: Dalton’s law of partial pressure states that the sum of partial pressures of all gases present in…

Q: A liter of methane gas, CH4, at STP contains more atoms of hydrogen than does a liter of pure…

A: Given,  Volume of CH4 gas = 1.0 L  Volume of H2 gas = 1.0 L  Condition of the reaction = STP…

Q: A gaseous compound has a density of 1.40 g/L at 21.8 °C and 1.34 atm. What is the molar mass of the…

A: Given:: Density d= 1.40 g L-1  T=21.8℃ = (21.8+273)K = 294.8 K P= 1.34 atm  Molar mass of compound =…

Q: At 750 K, a 296 mL container of Xe at 3.02 atm is connected by a valve to a 441 mL container of H2…

A: Ideal gas eequation can be written as: Here, P- pressure of gas V- volume of gas n- number of moles…

Q: If the mole fraction of He in a gas mixture is 0.545 and the total pressure of the gas is 882.4…

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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.