Stemson Kaiks
Mar 19
Nuetralization reaction 250ml of 0.6M sulphuric acid reaction 400ml of 0.5M potassium hydroxide solution. What is the limiting reactant?
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Mar 19
To determine the limiting reactant in this neutralization reaction, we need to compare the number of moles of each reactant present.
First, calculate the number of moles of sulphuric acid:
0.6 mol/L x 0.25 L = 0.15 moles
Next, calculate the number of moles of potassium hydroxide:
0.5 mol/L x 0.4 L = 0.2 moles
Since the number of moles of sulphuric acid (0.15 moles) is less than the number of moles of potassium hydroxide (0.2 moles), the limiting reactant in this reaction is the sulphuric acid.
First, calculate the number of moles of sulphuric acid:
0.6 mol/L x 0.25 L = 0.15 moles
Next, calculate the number of moles of potassium hydroxide:
0.5 mol/L x 0.4 L = 0.2 moles
Since the number of moles of sulphuric acid (0.15 moles) is less than the number of moles of potassium hydroxide (0.2 moles), the limiting reactant in this reaction is the sulphuric acid.
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