can someone help please


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What mass of the second-listed reactant in each of the following reactions is needed to react completely with 7.523 g of the first-listed reactant?

4NH3 + 5O2 → 4NO + 6H2O 

CaO + 3C → CO + CaC2 

Balance the reaction of sulfuric acid with sodium hydroxide.

H2SO4 + NaOH → Na2SO4 + H2O

How many moles of sodium sulfate are produced when 33.3 moles of sodium hydroxide completely react with sulfuric acid.

Nov 18th, 2017

1) 7.523g O2 * (1mol/16g O2) =.470188mol O2

    .470188 mol 02 * (4 mol NH3/5mol O2) = .37815 mol NH3

    .37815 mol NH3 * (17.034g NH3/ 1 mol NH3) = 6.407g NH3 (with proper sig. figs.)

2)7.523g  C *(1 mol/12.0107g C) = .62636 mol C

   .62636 mol C * (1 mol CaO/3 mol C) = .20879 mol CaO

   .20879 mol Ca) * (56.078g/mol) = 11.71g CaO

3) H2SO4 + 2 NaOH -> Na2SO4 + 2 H2O

   33.3 mol NaOH * (1 mol Na2SO4 / 2 mol NaOH) = 16.65 mol Na2SO4



A good resource with which you could learn how to do these problems is: https://www.youtube.com/watch?v=UL1jmJaUkaQ

Dec 11th, 2014

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