#H_2SO_4 + 2LiOH -> Li_2SO_4 + 2H_2O# What mass of water is produced from 10 g of sulfuric acid?

Answer 1

Approx. #4*g#.

#"Moles of sulfuric acid"# #=# #(10.0*cancelg)/(98.08*cancelg*mol^-1)=0.102*mol.#

Now we have the molar quantity of sulfuric acid that react; we also have the stoichiometric equation that shows the molar equivalence of sulfuric acid, and lithium hydroxide.

Given the stoichiometry, #"mass of water"# #=# #0.102*molxx2xx18.01*g*mol^-1=??*g#.

Why did I multiply the mass in this equation by #2#? Am I pulling your leg?

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Answer 2

Avery Adams

To calculate the mass of water produced from 10 g of sulfuric acid (H2SO4), we first need to determine the molar mass of H2SO4, which is 98.08 g/mol.

From the balanced chemical equation, we can see that 1 mole of H2SO4 produces 2 moles of water (H2O).

Using the molar mass of water (18.02 g/mol), we can calculate the mass of water produced from 10 g of sulfuric acid:

10 g of H2SO4 * (1 mol / 98.08 g) * (2 mol H2O / 1 mol H2SO4) * (18.02 g / 1 mol) = 3.66 g of water

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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.

#H_2SO_4 + 2LiOH -&gt; Li_2SO_4 + 2H_2O# What mass of water is produced from 10 g of sulfuric acid?

#H_2SO_4 + 2LiOH -> Li_2SO_4 + 2H_2O# What mass of water is produced from 10 g of sulfuric acid?