Question

Помогите решить задачи с оформлением 1. Какое количество теплоты выделиться для сгорания 44г водорода, если известно термохимическое уравнение реакции: H2+O2= H2O + 646кДж 2. Какое количество углерода сгорело в кислороде, если известно, что при сгорании этого количества углерода выделилось 980кДж теплоты. Используйте термохимическое уравнение: С+О2 = СО +340кДж 3. В результате взаимодействия алюминия с кислородом выделилось 3695кДж теплоты. Какова масса кислорода, участвовавшего в реакции? Используйте термохимическое уравнение: Аl + O2 = Al2O3 + 870кДж срочно

Answer 1

Ответ:

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Answer 2

Task 1: Quantity of Heat Released in the Combustion of Hydrogen

To find the quantity of heat released in the combustion of 44g of hydrogen, we can use the given thermochemical equation:

H2 + O2 → H2O ΔH = -646 kJ

The negative sign indicates that the reaction is exothermic, meaning it releases heat.

To calculate the quantity of heat released, we need to determine the number of moles of hydrogen in 44g. The molar mass of hydrogen (H2) is 2 g/mol.

Step 1: Calculate the number of moles of hydrogen: Number of moles = Mass / Molar mass Number of moles = 44g / 2 g/mol = 22 mol

Step 2: Use the stoichiometric coefficients from the balanced equation to determine the quantity of heat released: Quantity of heat released = ΔH * Number of moles of hydrogen Quantity of heat released = -646 kJ/mol * 22 mol = -14,212 kJ

Therefore, the quantity of heat released for the combustion of 44g of hydrogen is 14,212 kJ. [[1]]

Task 2: Quantity of Carbon Burned in Oxygen

To find the quantity of carbon burned in oxygen, given that 980 kJ of heat is released, we can use the given thermochemical equation:

C + O2 → CO ΔH = -340 kJ

Again, the negative sign indicates an exothermic reaction.

To calculate the quantity of carbon burned, we need to determine the number of moles of carbon that corresponds to 980 kJ of heat released.

Step 1: Calculate the number of moles of carbon: Quantity of heat released = ΔH * Number of moles of carbon Number of moles of carbon = Quantity of heat released / ΔH Number of moles of carbon = 980 kJ / -340 kJ/mol ≈ -2.88 mol

Since the number of moles cannot be negative, we take the absolute value.

Step 2: Convert the number of moles of carbon to grams: Mass of carbon = Number of moles * Molar mass Mass of carbon = 2.88 mol * 12 g/mol = 34.56 g

Therefore, the quantity of carbon burned in oxygen is approximately 34.56 g. [[2]]

Task 3: Mass of Oxygen Involved in the Reaction

To find the mass of oxygen involved in the reaction, given that 3695 kJ of heat is released, we can use the given thermochemical equation:

2Al + 3/2O2 → Al2O3 ΔH = -870 kJ

Once again, the negative sign indicates an exothermic reaction.

To calculate the mass of oxygen involved, we need to determine the number of moles of oxygen that corresponds to 3695 kJ of heat released.

Step 1: Calculate the number of moles of oxygen: Quantity of heat released = ΔH * Number of moles of oxygen Number of moles of oxygen = Quantity of heat released / ΔH Number of moles of oxygen = 3695 kJ / -870 kJ/mol ≈ -4.25 mol

Since the number of moles cannot be negative, we take the absolute value.

Step 2: Convert the number of moles of oxygen to grams: Mass of oxygen = Number of moles * Molar mass Mass of oxygen = 4.25 mol * 32 g/mol = 136 g

Therefore, the mass of oxygen involved in the reaction is approximately 136 g. [[3]]

I hope this helps! Let me know if you have any further questions.