Solid iron reacts with sulfuric acid to produce iron (ll) sulfate and hydrogen gas. If 655 mL gas are collected at STP, how many grams of iron (II) sulfate are also produced?

Answer 1

Caleb Adams

#Fe(s) + H_2SO_4(aq) rarr FeSO_4(aq) + H_2(g)uarr#

It is a fact that at STP, 1 mole of ideal gas (whose behaviour should approximate) has a volume of #22.4# #L#.

We have #0.655# #L# produced by the reaction; i.e. #(0.655*cancelL)/(22.4*cancelL*mol^-1)# #=# #0.292# #mol#.

By stoichiometry there must have been #0.292# #mol# #xx# #151.9*g*mol^-1# #=# #??g# #FeSO_4#.

Sign up to view the whole answer

By signing up, you agree to our Terms of Service and Privacy Policy

Sign up with email

Answer 2

Axel Alvarado

First, we need to calculate the number of moles of hydrogen gas produced using the ideal gas law at STP (Standard Temperature and Pressure):

1 mole of any gas occupies 22.4 liters at STP.

Given that 655 mL (or 0.655 L) of hydrogen gas is collected, we can calculate the number of moles of hydrogen gas produced:

moles of H₂ = (volume of gas collected) / (molar volume at STP) = 0.655 L / 22.4 L/mol ≈ 0.0292 moles of H₂

The balanced chemical equation for the reaction tells us that 1 mole of iron reacts with 1 mole of sulfuric acid to produce 1 mole of iron(II) sulfate and 1 mole of hydrogen gas.

So, the number of moles of iron(II) sulfate produced is also approximately 0.0292 moles.

Next, we need to calculate the molar mass of iron(II) sulfate (FeSO₄):

Iron (Fe): 55.85 g/mol Sulfur (S): 32.07 g/mol Oxygen (O): 16.00 g/mol

Molar mass of FeSO₄: = (1 * Fe) + (1 * S) + (4 * O) = (1 * 55.85) + (1 * 32.07) + (4 * 16.00) = 55.85 + 32.07 + 64.00 = 151.92 g/mol

Now, using the number of moles of iron(II) sulfate and its molar mass, we can calculate the mass of iron(II) sulfate produced:

mass of FeSO₄ = (number of moles) * (molar mass) ≈ 0.0292 moles * 151.92 g/mol ≈ 4.44 grams

So, approximately 4.44 grams of iron(II) sulfate are produced.

Sign up to view the whole answer

By signing up, you agree to our Terms of Service and Privacy Policy

Sign up with email

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.