Question

Химия!!!! ЗАДАЧИ!!! Ребят, хэлп плиз. я просто НЕ ШАРЮ Вычислите массу цинка, образовавшегося при восстановлении его углём из оксида массой 810 гВычислите объём угарного газа, образующегося при взаимодействии оксида цинка с углём массой 12, 63 г, содержащим 5% неуглеродных примесейКакой объём при нормальных условиях займёт углекислый газ, получающийся при сгорании 224, 5 г угля, содержащего 2% неуглеродных примесей Ребят, пожалуйста, с дано и лучше прикрепите фотографию с решением

Answer 1

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Answer 2

Mass of Zinc Formed:

To calculate the mass of zinc formed during the reduction of zinc oxide with carbon, we need to use the stoichiometry of the reaction and the given mass of zinc oxide.

The balanced chemical equation for the reaction is: ZnO + C → Zn + CO

According to the equation, 1 mole of zinc oxide reacts with 1 mole of carbon to produce 1 mole of zinc. The molar mass of zinc is 65.38 g/mol.

Given that the mass of zinc oxide is 810 g, we can calculate the number of moles of zinc oxide using its molar mass (81.38 g/mol): moles of ZnO = mass of ZnO / molar mass of ZnO = 810 g / 81.38 g/mol = 9.95 mol

Since the stoichiometry of the reaction is 1:1, the number of moles of zinc formed is also 9.95 mol.

To calculate the mass of zinc formed, we multiply the number of moles of zinc by its molar mass: mass of Zn = moles of Zn × molar mass of Zn = 9.95 mol × 65.38 g/mol = 650.81 g

Therefore, the mass of zinc formed during the reaction is approximately 650.81 grams.

Volume of Carbon Dioxide Gas Formed:

To calculate the volume of carbon dioxide gas formed during the reaction between zinc oxide and carbon, we need to use the ideal gas law and the given mass of carbon.

The balanced chemical equation for the reaction is: ZnO + C → Zn + CO

According to the equation, 1 mole of carbon dioxide is produced for every mole of carbon used. The molar mass of carbon dioxide is 44.01 g/mol.

Given that the mass of carbon is 12.63 g and it contains 5% impurities, we can calculate the mass of pure carbon: mass of pure carbon = mass of carbon × (100% - % impurities) = 12.63 g × (100% - 5%) = 11.99 g

Next, we calculate the number of moles of pure carbon using its molar mass (12.01 g/mol): moles of pure carbon = mass of pure carbon / molar mass of carbon = 11.99 g / 12.01 g/mol = 0.998 mol

Since the stoichiometry of the reaction is 1:1, the number of moles of carbon dioxide formed is also 0.998 mol.

To calculate the volume of carbon dioxide gas formed, we use the ideal gas law equation: PV = nRT

Assuming the reaction takes place at standard temperature and pressure (STP), where T = 273.15 K and P = 1 atm, we can rearrange the equation to solve for volume (V): V = nRT / P = (0.998 mol) × (0.0821 L·atm/(mol·K)) × (273.15 K) / (1 atm) = 22.2 L

Therefore, the volume of carbon dioxide gas formed during the reaction is approximately 22.2 liters.

Volume of Carbon Dioxide Gas at Normal Conditions:

To calculate the volume of carbon dioxide gas at normal conditions (0 °C and 1 atm), we can use the combined gas law.

Given that the initial volume of carbon dioxide gas is 22.2 L and the initial conditions are STP, we can use the combined gas law equation: (P1 × V1) / T1 = (P2 × V2) / T2

Substituting the values: P1 = 1 atm (initial pressure at STP) V1 = 22.2 L (initial volume at STP) T1 = 273.15 K (initial temperature at STP) P2 = 1 atm (final pressure at normal conditions) V2 = ? T2 = 273.15 K (final temperature at normal conditions)

Simplifying the equation: (1 atm × 22.2 L) / 273.15 K = (1 atm × V2) / 273.15 K

Solving for V2: V2 = (1 atm × 22.2 L) / 273.15 K = 0.0812 L

Therefore, the volume of carbon dioxide gas at normal conditions is approximately 0.0812 liters.

Unfortunately, I am unable to attach a photo of the solution, but I hope the provided explanations are clear and helpful.