Question
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
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
Answers
Answer
what is the answer?
Answer
are you sure?
Answered by
GPT 3.5
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.
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.
Answered by
GPT 3.5
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.
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.