Question

Какой объем водорода (н.у.) выделится при действии на цинк массой 32.5 на избыток серной кислоты?

Answer 1

32,5 г                                                                  Х л
 Zn        +        H2SO4      ->      ZnSO4      +      H2
n = 1 моль                                                        n = 1 моль
М = 65 г/моль                                                  Vm=22,4 л/моль
m = 65 г                                                            V = 22,4 л
32,5 г Zn    -    Х л Н2
65 г Zn      -    22,4 л Н2
V(H2) = 32,5 * 22,4 / 65 = 11,2 л

Answer 2

Calculating the Volume of Hydrogen Gas Produced

To calculate the volume of hydrogen gas produced when 32.5 grams of zinc reacts with an excess of sulfuric acid, we can use the stoichiometry of the balanced chemical equation for the reaction between zinc and sulfuric acid.

The balanced chemical equation for the reaction is: Zn + H2SO4 → ZnSO4 + H2

According to the stoichiometry of the balanced chemical equation, 1 mole of zinc reacts with 1 mole of sulfuric acid to produce 1 mole of hydrogen gas.

Step 1: Calculate the Moles of Zinc

To find the moles of zinc, we can use the molar mass of zinc, which is 65.38 g/mol.

Moles of zinc = Mass of zinc / Molar mass of zinc Moles of zinc = 32.5 g / 65.38 g/mol Moles of zinc ≈ 0.497 moles

Step 2: Calculate the Moles of Hydrogen Gas

Since the stoichiometry of the balanced chemical equation is 1:1 for zinc and hydrogen gas, the moles of hydrogen gas produced will be the same as the moles of zinc reacted.

Moles of hydrogen gas = Moles of zinc Moles of hydrogen gas ≈ 0.497 moles

Step 3: Convert Moles to Volume at Standard Temperature and Pressure (STP)

At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters.

Volume of hydrogen gas at STP = Moles of hydrogen gas × 22.4 L/mol Volume of hydrogen gas at STP ≈ 0.497 moles × 22.4 L/mol Volume of hydrogen gas at STP ≈ 11.15 liters

Therefore, approximately 11.15 liters of hydrogen gas will be produced when 32.5 grams of zinc reacts with an excess of sulfuric acid.

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