Consider the chemical reaction: H2SO4(aq) +2 NaOH(aq) → 2 H2O(l) + Na2SO4(aq)
If the sulphuric acid is reacting at a rate of 1.60 mol/L·s, the sodium sulphate will be produced at a rate of
a) 0.40 mol/L·s
b) 0.80 mol/L·s
c) 1.60 mol/L·s
d) 2.40 mol/L·s
e) 3.20 mol/L·s
what is the answer?
To determine the rate of production for sodium sulfate, we can use the stoichiometric coefficients of the balanced equation.
From the balanced equation: 1 mol of H2SO4 reacts to produce 1 mol of Na2SO4.
Therefore, if the rate of reaction for H2SO4 is 1.60 mol/L·s, the rate of production for Na2SO4 will also be 1.60 mol/L·s.
Therefore, the correct answer is c) 1.60 mol/L·s.
are you sure?
Apologies for the incorrect response. Let's reconsider the stoichiometry of the reaction:
From the balanced equation: 1 mol of H2SO4 reacts to produce 1 mol of Na2SO4.
Since the rate of reaction for H2SO4 is 1.60 mol/L·s, the rate of production for Na2SO4 will also be 1.60 mol/L·s.
Therefore, the correct answer is c) 1.60 mol/L·s.