WebExample #8: A mixture of 14.0 grams of hydrogen, 84.0 grams of nitrogen, and 2.00 moles of oxygen are placed in a flask. When the partial pressure of the oxygen is 78.00 mm of mercury, what is the total pressure in the flask? Solution: 1) Determine the moles of each gas: nitrogen ---> 84.0 g / 28.014 g/mol = 2.9985 mol WebIn the combustion of hydrogen gas, hydrogen reacts with oxygen from the air to form water vapor. Hydrogen + Oxygen Yields Water. If you burn 47.8 g of Hydrogen and produce 427 g of water, how much oxygen reacted? Subtract g of Water with g of Hydrogen and you get 379.2 g of Oxygen
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WebMar 27, 2024 · One of them is the number of moles which is a bit outside the scope of thermodynamics. The other three are pressure, temperature, and volume. We can … WebOct 23, 2015 · Oxygen. Explanation: Start by taking a look at the balanced chemical equation for this reaction 2H2 (g] +O2 (g] → 2H2O(l] Notice that you have a 2:1 mole ratio between hydrogen gas and oxygen gas. This means that, regardless of how many moles of oxygen gas you have, the reaction needs twice as many moles of hydrogen gas in order … i love the cocaine buckcherry
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WebApr 4, 2024 · Kinetic theory of Gases Answer In a cylinder there are 60 g Ne and 64 g Oxygen ( O 2) . If the pressure of the mixture of gases in cylinder is 30 bar then the … Weboxygen in product therefore it follows the law of conservation of mass. (ii) The total mass of reactants = total mass of product; therefore, the law of multiple proportions is followed. (iii) Amount of Fe2O3 can be increased by taking any one of … WebCalculate the volume of gaseous NO₂ produced by the combustion of 100 g of NH₃ at 0°C and 100 kPa. Solution Step 1. Write the balanced chemical equation. 4NH₃ (g) + 7O₂ (g) → 4NO₂ (g) + 6H₂O (l) Step 2. Convert mass of NH₃ → moles of NH₃ → moles of NO₂. 100 g NH₃ × 1mol NH3 17.03g NH3 × 4mol NO2 4mol NH3 = 5.872 mol NH₃ (3 significant … i love the captain