How many liters of NH3 can be produced at 11 atm and 24 °C from a 3 g sample of nitrogen gas and an excess of hydrogen gas? N2(g) -3H2(g) ---> 2NH3(g) +

Q: Magnesium reacts with water as follows: Mg(s) + 2 H2O(1) Mg(OH)2(s) + H2(g) (balanced) If 5.60 g of…

A: To solve these problems, we will follow these steps:1.  Percent Yield Calculation1. Balanced…

Q: 584 grams of sugar, how many liters of CO2

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Q: Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen…

A: Given,Mass of NH3 = 5.28 gMass of HCl = 5.28 gMoles of NH3 and HCl can be calculated as:

Q: Use the ideal gas law to calculate an unknown property. A sample of O₂ gas has a volume of 811 mL,…

A: Given - Volume of O2 =811 mL = 0.811 L  (1L = 1000ml) Pressure of O2= 41 mmHg  Temperature =13.6 °C…

Q: Consider the following chemical reaction: C(s)+H2O(g)→CO(g)+H2(g) How many liters of hydrogen gas…

A: Given: mol of Carbon = 1.07 mol pressure = 1 atm temperature = 317 K we have to find grams of carbon…

Q: (For #5-7) Acetylene (C2H2) is formed by the reaction of water with calcium carbide, according to…

A:

Q: An ideal gas in a sealed container has an initial volume of 2.65 L. At constant pressure, it is…

A: We have initial volume of gas as 2.65 L Final temperature is 25°C Final volume is 1.75 L Initial…

Q: CaO(s) + CO2 (g) → CaCO3 (s) What mass of CO2 could be absorbed by 1.95 g of CaO? Mass = g CO2 What…

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Q: What volume of ammonia gas at 563 K and 1.61 atm can be produced from the reaction of 1.60 kg of…

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Q: What volume of hydrogen gas (in mL) at 703 mm Hg and 40 °C can be produced when 2.9 g of MgCO3(s)…

A: According to an ideal gas equation PV= nRT Where P= pressure of the gas, V= volume of the gas, n= no…

Q: A) A 3.50 liter metal cylinder contains only ethane gas, C2H6. If the pressure in the container is…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Wine goes bad soon after opening because the ethanol  CH3CH2OH in it reacts with oxygen gas  O2…

A: Consider the reaction fr the given condition is as follows; Reaction:        CH3CH2OH     +     O2…

Q: What volume of hydrogen gas, in mL, is produced from 0.128 g Mg reacting with an excess of HCI at a…

A: A question based on the mole concept. Using the information about the number of moles of reactant…

Q: filled it with the gas at 1.00 atm and 21.0 °C and weighed it again. The difference in mass was 3.5…

A: The question is based on concept of  gaseous state.  We have to identify the gas which is present in…

Q: W hat volume of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of…

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Q: What is the molarity of a HClHCl solution if the reaction of 215. mLmL of the HClHCl solution with…

A: The concentration of a solution is a measure of the amount of solute that has been dissolved in a…

Q: O A tank contains nitrogen N2 at an absolute pressure of 2.5 atm. What will be the pressure of an…

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Q: Phosphorus pentachloride decomposes according to the chemical equation…

A: The equilibrium constant denoted by the symbol ‘K’ can be defined as a number which is used to…

Q: A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas city (MCI) to…

A: Given data,Mass of fuel=11800lbwe know,1lb=453.592gMass of fuel=11800×453.592g=5352390gC:H=1:2

Q: CuSO4 (aq) + Zn(s) → Cu(s) + ZnSO4(aq) The single-replacement reaction above produces 140.0 g of…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: . A gaseous hydrocarbon, in a volume of 25.4 L at 400 Kand a pressure of 3.40 atm, reacts in an…

A: Moles of gaseous hydrocarbon, n= PVRT = 3.40 x 25.4 0.0821 X 400 = 2.63 mol Moles of Carbon atoms =…

Q: In the preparation of 60 mL Magnesium citrate in the laboratory, you are required to: calculate for…

A: Given: Mass of magnesium carbonate used = 2.57 g. Moles of magnesium carbonate reacting = MassMolar…

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.