# 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?

##### 2 Answers

Mar 15, 2016

#### Answer:

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

Answer is 355 grams.

#### Explanation:

Given the molecular weights:

The analogy of the moles will be held constant:

For each one, substitute:

Therefore:

Mar 15, 2016

#### Answer:

Through conversion method using mole ratio and formula masses the answer is

#### Explanation:

- 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# .