A balloon filled with NO2 (g) has an initial volume of 8 L.  If half the NO2 reacts to form N2O4 (g) at constant temperature and pressure, what is the final volume (L) of the balloon?

Q: 2. If 1.0 x 103 g uranium metal is converted to gaseous UF6, calculate the pressure of UF6 at 62°C…

A: The combined gas legislation incorporates three gas legislation: the law of Boyle, Charles' law and…

Q: At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH₂) and propane (C₂H₂) was burned, producing…

A: We have to calculate the mole fraction of methane and propane

Q: Consider the following balanced reaction: 2 H₂S(g) +30₂(g) →2 H₂O(1) +2 SO 2(g) 5.00 L of H₂S and…

A:

Q: 4.00 L flask contains 1.40 atm argon at 25°C. a) Calculate the moles of argon gas initially present…

A: We will calculate all parts

Q: The pressure of a sample of argon gas was increased from 1.86 atm to 6.70 atm at constant…

A:

Q: A 0.101 mol sample of O2 gas is contained in a 3.00 L flask at room temperature and pressure. What…

A:

Q: You are asked to design an air bag for a car. You know that the bag should be filled with gas with a…

A:

Q: In a common Freshman College Laboratory experiment, KClO3 is decomposed by  heating to give KCl and…

A: Answer:- Firstly a balanced chemical equation is written then using the simple concept of…

Q: When 44.5 L of nitric oxide reacts with 38.2 L of oxygen at 423 K under a constant pressure of 1.03…

A: We have given that  When 44.5 L of nitric oxide reacts with 38.2 L of oxygen at 423 K under a…

Q: A bottle with the volume 4.03 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr…

A:

Q: A sample of butane (C4H10) gas having a volume of 2.0 L at 25 °C and 1300 mm Hg was mixed with a…

A: PFA

Q: What volume of ammonia (NH)3 is formed if 8.84 x 10^21 molecules of carbon dioxide are also produced

A: Interpretation -  To determine the volume of ammonia NH3 is formed if 8.84 x 10^21 molecules of…

Q: The oxidation of trichloroethane results in the following reaction equation: 4 CaH,C|a() + 11 0, (g)…

A:

Q: Suppose we have a 12.2 L sample containing 0.50 mol oxygen gas (O2) at a pressure of 1 atm and a…

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Q: 3. Calculate the pressure inside a tube, given that the tube's volume is 4.0 L, its temperature is…

A:

Q: A magnesium with a mass of 0.06581 grams was reacted with excess HCl. The reaction produced 51.12 mL…

A: The balanced chemical reaction reaction is  Mg (s)     +    2 HCl (aq)     -------->     MgCl2…

Q: The volume of a sample of pure HCl gas was 289 mL at 24 ° C and 137 mmHg. It was completely…

A: The number of moles of HCl is calculated as,

Q: Consider the following reaction: 2 NH3 (g)   +   3 Cl2 (g)   →   N2 (g)   +   6 HCl (g) A mixture…

A: Consider the following reaction: 2 NH3 (g)   +   3 Cl2 (g)   →   N2 (g)   +   6 HCl (g) The given…

Q: Zn reacts with hydrochloric acid to give zinc chloride and hydrogen gas. A sample of 5 g of a Zn…

A: Final answer is in the attachmentExplanation:Step 1:First, we need to find the equation that…

Q: Determine the mass, in kg, of HgO that must decompose to form 78.4 L O2 gas at STP.    2HgO(s) →…

A: To solve this problem we have to calculate the mass of HgO .

Q: How much volume is occupied by 94.0 g of SO 2 STP

A: Volume = 32.86 Letter

Q: A 2.50 L sample of butane gas (C4H10), measured at 22.0 ºC and 1.20 atm pressure, is combusted…

A: Given Initial volume of butane gas = 2.50 L Temperature = 22.0°C = 295K Pressure = 1.20 atm Volume…

Q: 13. If 3.5 kg of Fe is produced by the following reaction, what volume, at STP, of CO2 would be…

A: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)  Given mass Fe produced = 3.5 Kg =3500 g Number of moles of Fe…

Q: Zn reacts with hydrochloric acid to give zinc chloride and hydrogen gas. A sample of 5 g of a Zn…

A: To solve the given problem, let's break it down into three parts:a) Finding the mass of zinc…

Q: A 0.477 mol sample of O gas has a volume of 12.8 L at a certain temperature and pressure. If all…

A: NOTE : In the reaction, the subscripts are missing. Hence I'm considering correct reaction. The…

Q: Predict the number of molecules for diatomic gas, X, if the volume at STP is 44.80 L. [Molar volume…

A: We have to calculate the number of molecules for gas.

Q: The pressure of a sample of argon gas was increased from 1.76 atm to 6.60 atm at constant…

A: At constant temperature volume of gas is inversely proportional to pressure

Q: At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C3Hg) was burned, producing…

A:

Q: In a common Freshman College Laboratory experiment, KClO3 is decomposed by heating to give KCl and…

A: 2 KClO3 ---> 2 KCl + 3O2  Volume of O2 = 0.238 L  Temperature = 28°C  Pressure = 752 mm Hg 760 mm…

Q: Determine the mass, in kg, of HgO that must decompose to form 52.9 L O2 gas at STP.    2HgO(s) →…

A:

Q: A sample of gas was enriched to contain 2 % by mass of 15N with the remainder being 14N. Calculate…

A: • Average Atomic mass = Σ Mass of isotopes x Fraction of abundance• Molar mass of N2O = 2 x Atomic…

Q: . Ammonia gas is produced by the reaction: N2(g) + 3H2(g) → 2NH3 (g).  (a) How many liters of…

A: The balanced reaction given is, => N2 (g) + 3 H2 (g) ------> 2 NH3 (g)

Q: a 12.2-L sample containing 0.50 mol O2 gas at a pressure of 1 atm and a temperature of 25 celsius.…

A: Given: moles of O2 = 0.50 mol          ( V =  12.2 L ,P = 1atm ,T = 25 celcius = 298K) From the…

Q: How many argon atoms are contained in 7.66 x 105 mmol of argon? 4.61 x 1026 Ar atoms 1.84 x 1028 Ar…

A: Given, moles of argon = 7.66 x 105 mmol  we know, 1 mol = 1000 millimole(mmol) => moles of argon…

Q: What volume of NH3 (measured at STP) can be produced by reacting 8.51 liters (STP) N2 with 3.15 x…

A: Use stoichiometry of the equation to get the answer.

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.