Anonymous
Anonymous asked in Science & MathematicsChemistry · 8 months ago

chemistry ?

Determine the chemical amount (moles) of silver produced when 210 g of silver nitrate completely reacts with tin, as shown in the following reaction equation:

Sn(s) + 2AgNO3(aq) → 2Ag(s) + Sn(NO3)2(aq 

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The production of ammonia is given by the equation:

3H2(g) + N2(g) → 2NH3(g)

 If 5.0 g of hydrogen reacts with excess nitrogen, how much ammonia will be produced? 

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Consider the following unbalanced reaction equation: Al2O3(s) + H2(g) → Al(g) + H2O(g)

When this equation is correctly balanced, the coefficient of 

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Potassium chloride and oxygen gas are formed upon heating potassium chlorate. The following balanced equation shows this decomposition process:

2KClO3(s) → 2KCl(s) + 3O2(g)

The chemical amount of KClO3 required to produce 5.0 mol of oxygen is: 

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Calculate the mass of precipitate (solid) produced when 75 mL of 6.00 mol/L sodium hydroxide solution is reacted with excess aluminum nitrate solution.

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A company is recycling expensive silver metal from a concentrated silver nitrate solution. Consider the following skeleton (unbalanced) equation:

AgNO3(aq) + Cu(s) → Cu(NO3)2(aq) + Ag(s)

What are the coefficients required, in order from left to right, to balance this equation? 

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if the theoretical yield of a particular reaction is 23 g and the percent yield is 87%, what is the actual yield? 

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1 Answer

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  • 8 months ago
    Favorite Answer

    only one question allowed, you have 7.

    I'll do one

    Hydrogen + Nitrogen ➜ Ammonia

    3H₂ + N₂ ➜ 2NH₃

    molecular weights

    H = 1

    N = 14

    3H₂ = 6

    N₂ = 2•14 = 28

    2NH₃ = 2•17 = 34

    check 6 + 28 = 34

    3 mole of H₂ + 1 moles of N₂ ➜ 2 moles of NH₃

    6 grams of H₂ + 28 grams of N₂ ➜ 34 grams of NH₃

     If 5.0 g of hydrogen reacts with excess nitrogen, how much ammonia will be produced? 

    ratio ammonia to hydrogen is 34/6

    34/6 = x/5

    x = 28 g

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