The total pressure in the container is 0.950 atm at 25°C before the reaction. What is the final pressure in the container at 125°C after the reaction, assuming an 88.0% yield and no volume change? A mixture in which the mole ratio of hydrogen to oxygen is 2:1 initially is used to prepare water using the reaction below. 2 H20 (g) + O2 (g) → 2 H20 (g)

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A: Mass of magnesium = 0.0294 grams Temperature  of Hydrogen gas = 25.9°C  or 299.05K partial pressure…

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Q: Calculate the volume of 1.62g of Helium gas at 25.670C and 872 mmHg.  (R = 0.0821 atm.L/mol.K

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A: Given that  composition in percent by volume: 9.26 CO2, 22.0% CO , 17.5%H2, 3.3% CH4 and 48.0% N2.

Q: Please don't provide handwritten solution ....

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Q: What volume of CO₂ gas at 1.000 atm and 800 K could be produced by the reaction of 45.0 g of CaCO,…

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Q: 1) Calculate the volume of 1.62g of Helium gas at 25.670C and 872 mmHg.  (R = 0.0821 atm.L/mol.K)

A: As per our guidelines, we are supposed to answer?️ only one question. Kindly repost other questions…

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Q: A 2.20 L container at 53.6 °C contains 6.21g N2⁢O3⁡(g). The N2⁢O3 gas decomposes completely,…

A: Given :  Volume of vessel = 2.20 L  Temperature = 23.6 °C = 296.6 K  Mass of N2O3 = 6.21 g

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.