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A:
Q: How many moles of H2 are required to produce 5 moles of NH3? * N₂ 6.5 2.5 6.75 O 7.5 + H₂ NH3
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3/5= 0.6 moles of CO2 can be produced from one mole os O2
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- Air Pollution Nitrogen monoxide, which is present in urban air pollution, immediately Converts to nitrogen dioxide as it reacts with oxygen. a. Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen monoxide. b. What mole ratio would you use to convert from moles of nitrogen monoxide to moles of nitrogen dioxide?P4O10 + KOH → K3PO4 + H2Ois balanced, how much KOH is required toreact with 3 moles of P4O10?A 161 g sample of MnCl₂·nH₂O yields 112 g of the anhydrous compound after heating. Determine n in the chemical formula of the hydrate.
- Write the empirical formula for the hydrated KAl(SO4)2, based on moles of anhydrous KSI(SO4)2= 0.046 mol molar mass of H2O= 18g/ mol moles of H2O= 0.0444mol ratio pf moles H20 to moles of anhydrous KAI(SO4)2= 9.65/1 . Show all work including units. Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(SO4)2•4H2O.Calculate the moles of Be that can be contain from a 43.1 lb from a Be₃Al₂SiO₆?The principal component of mothballs is naphthalene, a compound with a molecular mass of about 130 amu, containing only carbon and hydrogen. A 3.000-mg sample of naphthalene burns to give 10.3 mg of CO2. Determineits empirical and molecular formulas.
- Ammonia is produced by the millions of tons annually foruse as a fertilizer. It is commonly made from N₂ and H₂ by theHaber process. Because the reaction reaches equilibrium beforegoing completely to product, the stoichiometric amount of am-monia is not obtained. At a particular temperature and pressure,10.0 g of H₂ reacts with 20.0 g of N₂ to form ammonia. When equilibrium is reached, 15.0 g of NH₃ has formed. (a) Calculatethe percent yield. (b) How many moles of N₂ and H₂ are presentat equilibrium?At the end of this, how did we go from a 5 to 1 ratio moles to 2CO2 and 3H2O?The following diagram represents a high-temperaturereaction between CH4 and H2O. Based on this reaction, findhow many moles of each product can be obtained startingwith 4.0 mol CH4. [Section 3.6]