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Interpretation:
The amount of ammonia formed if all of the limiting reactants were used up in Haber process then the yield obtained has to be named.
Concept Introduction:
Ratio of actual yield by theoretical yield multiplied by 100 gives percent yield. Percent yield equal to 100 % implies same actual and theoretical yield. Usually, percent yield is obtained below 100 % because actual yield lower in magnitude than theoretical value due to incomplete reactions and loss of sample during recovery.
The equation for percent yield is as follows:
percent yield = (actual yieldtheoretical yield)×100 %
Here,
Actual yield is quantity of product obtained from a
Theoretical yield is quantity of product obtained from balanced equation.
Units for actual and theoretical yield are same either in moles of grams.
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Chapter ST Solutions
Preparing for your ACS examination in general chemistry
- Don't used hand raiting and don't used Ai solutionarrow_forward2' P17E.6 The oxidation of NO to NO 2 2 NO(g) + O2(g) → 2NO2(g), proceeds by the following mechanism: NO + NO → N₂O₂ k₁ N2O2 NO NO K = N2O2 + O2 → NO2 + NO₂ Ко Verify that application of the steady-state approximation to the intermediate N2O2 results in the rate law d[NO₂] _ 2kk₁[NO][O₂] = dt k+k₁₂[O₂]arrow_forwardPLEASE ANSWER BOTH i) and ii) !!!!arrow_forward
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