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In the reaction #2NaOH+H_2SO_4 -> 2H_2O+Na_2SO_4#, how many grams of sodium sulfate will be formed if you start with 200.0 grams of sodium hydroxide and you have an excess of sulfuric acid?

Answer 1

Serenity Allen

Use the mole analogy of the reactant with the product. and substitute with the mole definition.

Answer is 355 grams.

The molecular weights being known:

#Mr_(NaOH)=40 g/(mol)# #Mr_(Na_2SO_4)=142 g/(mol)#

We will continue to use the mole analogy:

#n_(NaOH)/n_(Na_2SO_4)=2/1#

#n_(NaOH)/n_(Na_2SO_4)=2#

Replace each of them with:

#n=m/(Mr)#

Consequently:

#n_(NaOH)/n_(Na_2SO_4)=2#

#(m_(NaOH)/(Mr_(NaOH)))/(m_(Na_2SO_4)/(Mr_(Na_2SO_4)))=2#

#(200/40)/(x/142)=2#

#(200*142)/(40x)=2#

#200*142=2*40x#

#x=(200*142)/(2*40)=(100*142)/40=10*142/4=1420/4=#

#=710/2=355grams# (or just use a calculator)

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Answer 2

Jeremiah Adams

Through conversion method using mole ratio and formula masses the answer is #355# g of #Na_2SO_4#

Equation is already balanced, therefore what you need to find are the formula masses of the involved compounds, #NaOH# and #Na_2SO_4#;
Once known, start the calculation by converting #200# g #NaOH# to mole #NaOH# by multiplying it with the ratio of the formula mass of #NaOH#;
The result from the above calculation, will then be multiplied by the mole ratio of #Na_2SO_4# and #NaOH#, which is #(1 mol Na_2SO_4)/(2 mol NaOH)#;
Since, we are asked to find the mass of #Na_2SO_4# formed in this reaction, we need to multiply the answer of #step 3# to the ratio of the formula mass of #Na_2SO_4#.
Per calculation, the answer in mass is #355# grams of #Na_2SO_4#.

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Answer 3

Wyatt Adkins

To find the grams of sodium sulfate formed, first, calculate the moles of sodium hydroxide. Then, use the mole ratio from the balanced equation to find the moles of sodium sulfate. Finally, convert moles of sodium sulfate to grams.

Calculate moles of sodium hydroxide:
Moles = Mass / Molar mass
Moles of NaOH = 200.0 g / 40.00 g/mol = 5.00 moles
Use the mole ratio from the balanced equation:
2 moles NaOH : 1 mole Na2SO4
Moles of Na2SO4 = (5.00 moles NaOH) / 2 = 2.50 moles Na2SO4
Convert moles of Na2SO4 to grams:
Mass = Moles × Molar mass
Mass of Na2SO4 = 2.50 moles × (22.99 g/mol + 32.06 g/mol + (4 × 16.00 g/mol)) = 322.5 grams

Therefore, 322.5 grams of sodium sulfate will be formed.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

In the reaction #2NaOH+H_2SO_4 -&gt; 2H_2O+Na_2SO_4#, how many grams of sodium sulfate will be formed if you start with 200.0 grams of sodium hydroxide and you have an excess of sulfuric acid?

In the reaction #2NaOH+H_2SO_4 -> 2H_2O+Na_2SO_4#, how many grams of sodium sulfate will be formed if you start with 200.0 grams of sodium hydroxide and you have an excess of sulfuric acid?