2.8g of iron(¡¡) reacted with 100ml of 2M sulfuric acid. A.Which reactant is in exces? B. What volume of hydrogen gas is produce at RTP? C. How many moles of iron sulfate is produced? D. How many atoms of hydrogen gas were evolved?
A. Sulfuric acid B. O.01dm3 C. 0.03 moles D. 2*10^22 atoms
A. no. Fe + H2SO4 ==> FeSO4 + H2
2.8g Fe/55.85 = about 0.05 mols Fe.
mols H2SO4 = 0.1L x 2M = 0.2 mols.
0.05 mols Fe will form 0.05 mols FeSO4
0.2 mols H2SO4 2ill form 0.2 mols FeSO4(given all of the Fe it needs). Thw smaller number wins in all cases so Fe is the limiting reagent.
B. 0.05 mols H2 gas formed. That is 0.05 mols x 22.4 L/mol = ? L at STP. I don't know what RTP is so you will need to convert.
D. 1 mol contains 2*6.02E23 atoms. You had 0.05 mols; therefore, there are 0.05*2*6.02E23 atoms.
C.
A. To determine which reactant is in excess, we need to calculate the number of moles of each reactant and compare their stoichiometric ratios.
First, convert the mass of iron to moles using its molar mass. The molar mass of iron is approximately 55.85 g/mol.
2.8 g of iron x (1 mol / 55.85 g) = 0.05 moles of iron
Next, calculate the number of moles of sulfuric acid. The concentration of sulfuric acid is given as 2M (2 moles per liter). Since the volume is given in milliliters, we need to convert it to liters.
100 mL of sulfuric acid x (1 L / 1000 mL) = 0.1 L of sulfuric acid
Now, calculate the number of moles of sulfuric acid.
0.1 L of sulfuric acid x 2 mol/L = 0.2 moles of sulfuric acid
Comparing the moles of iron and sulfuric acid, we find that there are fewer moles of iron (0.05 moles) compared to sulfuric acid (0.2 moles). Therefore, iron is the limiting reactant and sulfuric acid is in excess.
B. To determine the volume of hydrogen gas produced at RTP (room temperature and pressure), we need to use the balanced chemical equation for the reaction between iron and sulfuric acid.
The balanced equation is:
Fe + H2SO4 -> FeSO4 + H2
From the balanced equation, it can be seen that one mole of iron reacts with one mole of sulfuric acid to produce one mole of hydrogen gas.
Since we know that there are 0.05 moles of iron, the same amount of moles of hydrogen gas will be produced.
The volume of one mole of any gas at RTP is approximately 22.4 liters. Therefore, the volume of hydrogen gas produced at RTP is:
0.05 moles of hydrogen x 22.4 L/mole = 1.12 L of hydrogen gas
C. To determine the number of moles of iron sulfate produced, we need to use the stoichiometry of the balanced equation.
From the balanced equation:
Fe + H2SO4 -> FeSO4 + H2
It can be seen that one mole of iron reacts with one mole of iron sulfate. Since we know there are 0.05 moles of iron, the same amount of moles of iron sulfate will be produced. Therefore, 0.05 moles of iron sulfate is produced.
D. To determine the number of atoms of hydrogen gas evolved, we need to use the Avogadro's number and the number of moles of hydrogen gas produced.
Avogadro's number is approximately 6.022 x 10^23 atoms/mol. Since we have calculated that 0.05 moles of hydrogen gas is produced, we can multiply the number of moles by Avogadro's number to get the number of atoms.
0.05 moles of hydrogen x 6.022 x 10^23 atoms/mol = 3.011 x 10^22 atoms of hydrogen gas