nickel container was charged with 0.814 atm of xenon gas and 1.26 atm of fluorine gas at 400°C. The xenon and fluorine react to form xenon tetrafluoride. What mass (g) of xenon tetrafluoride can be produced assuming 100% yield?

Q: Sodium azide, NaN3, decomposes according to the following equation and produces N2 gas that inflates…

A: Given, 2NaN3(s) ➝ 2Na(s) + 3N2(g) mass (in grams) of sodium azide (NaN3) needed = ? molar mass of…

Q: Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous…

A: Given reaction:  I₂(s) + 5F₂(g) → 2IF₅(g) The volume of the reaction flask = 10.00 L The mass of I₂…

Q: Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous…

A:

Q: The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the…

A: At STP- 1 mole gas = 22.4 L   Calculating moles of each gas by using dimensional analysis- 155 mL…

Q: Consider the following equation: CH&O7(s) +3 NaHCO3(s) + H20(1) --> Na3CgHgO7(s) + 3H2O(1) + 3CO2g)…

A: Here we first calculate the production of CO2 as a mole. Then use gas equation to determine the…

Q: You start with an equimolar mixture of the gases SO₂ and O₂ in a container. The SO₂ and O₂ react to…

A: Given data:

Q: A 20.0-L nickel container was charged with 0.828 atm of xenon gas and 1.25 atm of fluorine gas at…

A:

Q: A 15.0-L rigid container was charged with 0.500 atm of krypton gas and 1.50 atm of chlorine gas at…

A: Kr (g) + 2Cl2(g) ----> KrCl4(g) Temperature = 350°C = 623 K Volume = 15L Molar mass of Kypton…

Q: Aluminum trichloride is formed by reacting solid aluminum with chlorine gas. Calculate the percent…

A:

Q: When dinitrogen pentoxide gas reacts with nitrogen dioxide gas, the products are nitrogen monoxide…

A: According to the ideal gas equation, PV=nRTP=PressureV=Volumen=number of molesR=gas…

Q: How many moles of nitrogen gas are required to react completely with 19.8 L of oxygen gas according…

A: The chemical reaction is,                 N2 (g) + O2 (g)  ------> 2NO (g)   (Balanced) Thus one…

Q: What volume of a chlorine gas is required to react completely with 0.309 mol of bromine according to…

A:

Q: Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous…

A: Given mass of iodine = 11 g Molar mass of iodine = 253.81 g/mol Number of moles of iodine =…

Q: Hydrogen peroxide decomposes to form water and oxygen gas according to the following equation:…

A:

Q: 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of…

A:

Q: A vessel with a volume of 25.00 L contains 0.200 moles of nitrogen gas (N2), 0.300 moles of hydrogen…

A: Total Pressure in the vessel is equal to the sum of the partial pressure of the individual gases.…

Q: Isooctane (C8H18) is the primary component of gasoline, which burns according to the reaction below.…

A:

Q: When sodium chlorate (NaClO3) is heated, it decomposes into sodium chloride andoxygen gas. A student…

A: Given: V= 400 ml P = 0.931 atm T= 25 +273 = 298 K We have to calculate grams of  sodium chlorate? PV…

Q: What volume of oxygen gas is produced

A:

Q: 3 H2 (g) + N2 (g) --> 2 NH3 (g)   A 3.22 L vessel containing the hydrogen at 21.1 oC and 6.750 atm…

A: To determine the theoretical yield, we have to know the moles of reactants present initially. To get…

Q: When strongly heated, CaCO3 decomposes into carbon dioxide gas and calcium oxide. What mass of…

A:

Q: If a gaseous mixture is made by combining 2.17 g Ar and 2.55 g Kr in an evacuated 2.50 L container…

A:

Q: In the lab students reacted zinc with acid to generate and collect hydrogen gas, according to the…

A:

Q: What volume of hydrogen gas (in L) is produced when 0.381 moles of sodium reacts completely…

A: Moles of sodium=0.381 moles Temperature =35.2 °C=(35.2+273)K=308.2K Pressure=0.869atm R=0.0821…

Q: What volume of oxygen gas is produced when 40.9 g of mercury(II) oxide reacts completely according…

A: The equation for the dissociation of HgO is as follows, 2HgO (s) -> 2Hg (l) + O2 (g)  The…

Q: A gas mixture is made by combining 8.5 g8.5 g each of Ar,Ar, Ne,Ne, and an unknown diatomic gas. At…

A: According to ideal gas law PV = nRT where P = pressure V = volume n = moles R = gas constant =…

Q: Hydrazine, N2H4 reacts with oxygen to form nitrogen gas and water.  N2H4 (aq) +O2 (g) --->N2 (g) +…

A: 1 mole of Hydrazine reacts with oxygen to give 1 mole of nitrogen. The balanced chemical equation…

Q: The catalytic decomposition of hydrogen peroxide yields oxygen gas and water, according to the…

A: Given:Volume of hydrogen peroxide=75.3 mLTemperature= 25oCPressure=0.976 atmVolume of original…

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

A: The given chemical equation is: 2 HgO (s) → 2 Hg (l) + O2 (g) Given mass of HgO = 29.4 g  Molar mass…

Q: 4. A 30.6 g sample of gas occupies 22.414L at STP. What is the molecular weight of this gas?

A: As per the ideal gas equation: PV=nRT where, P = Pressure of gas V = Volume occupied by the gas n =…

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

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

Q: Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous…

A: Percentage of IF5 = 20.06 %

Q: Consider the following equation: C6H8O7(s)  + 3 NaHCO3(s) + H2O(l) --> Na3C6H8O7(s) + 3H2O(l) +…

A: Given mass of C6H8O7 = 193.6 molar mass of C6H8O7 = 192.1 g/mol Temperature = 313°K volume = 108.4 L

Q: ulfur burns in oxygen with a deep blue flame to produce sulfur dioxide.  If 5.85 g S8 and 1.00 atm…

A: Given : Mass of  S8 = 5.85 g  Pressure of 02 = 1 atm Volume = 5.00 L

Q: Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and…

A:

Q: When sulfur dioxide gas reacts with oxygen gas, sulfur trioxide forms.  1. If 3.5 moles of sulfur…

A:

Q: under thermal decomposition, potassium chlorate degrades into potassium chloride and oxygen by the…

A:

Q: Two gas tanks contain different gases. The pressure, volume, and temperature of eacn gas are shown…

A: Factors affecting the pressure of the gas: Volume- If the volume inside the container is decreased…

Q: A 4.00-g sample of a mixture of CaO and BaO is placed in a1.00-L vessel containing CO2 gas at a…

A: First we have to calculate the reacted pressure of CO2 gas in the given reaction:- The initial…

Q: What mass of potassium chloride forms when 5.25 L of chlorine gas at 0.950 atm and 293 Kelvin reacts…

A: It is given that 5.25 L of chlorine gas at a pressure of 0.950 atm at 293 K is reacting with 17 g of…

Q: What volume of sulfur dioxide is produced when 0.352 mol of hydrogen sulfide reacts completely…

A: Balanced reaction equation is :  2H2S + 3O2 -------> 2H2O + 2SO2    According to the balanced…

Q: The thermal decomposition of potassium chlorate can be used to produce oxygen in the laboratory.…

A:

Q: What volume of chlorine gas is required to react completely with 7.31x102 mol of carbon disulfide…

A: Ideal gas equation is, PV= nRT Where, P=pressure, V=Volume, n =number of moles R=gas constant…

Q: What volume of hydrogen gas is produced when 87.7 g of sodium reacts completely according to the…

A:

Q: Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous…

A: Volume of flask = V = 10.0 L Mass of I2 = 15.0 g  Pressure of F2 , P = 2.00 atm Temperature…

Q: A gas at 34C and 1.75 atm has a density of 3.4 g/L. Calculate the molar mass of the gas?

A: The ideal gas equation is given by,                               PV = nRT Where, P is the pressure…

Q: At 2.00oC and 1.00 atm, a sample of gas occupies 30.0 mL. If the temperature increases to 30.0oC and…

A:

Q: A 18.0 mg sample of an unknown gas is placed in a 750.0 mL flask at 85 0C and 1.20 atm. What is the…

A: Given data,Mass of gas=18.0mg=0.018gVolume=750mL=0.750LTemperature=85oC=85+273=358KPressure=1.2atm

Q: At 1.041.04 atm and 6.78 ∘C6.78⁢ ∘C, a 3.543.54 g sample of gas occupies a volume of…

A:

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.