Question

Помогите решить задание по химии В результате реакции,термохимическое уравнение которой 2SO2(г.)+О2(г.)=2SO3(г.) + 198 кДж,выделилось 1980 кДж теплоты.Количество израсходованого оксида (IV) равно 1) 5 моль 3) 10 моль 2)1 моль 4) 20 моль Решите пожалуйста с решением

Answer 1

Помогла бы решить но я в 3 классе у нас нет химии

Answer 2

Task Analysis

The task requires solving a chemistry problem related to a thermochemical equation. The given equation is:

2SO2(g) + O2(g) = 2SO3(g) ΔH = -198 kJ

It is also mentioned that 1980 kJ of heat is released during the reaction. The task is to determine the amount of oxide (IV) consumed, given four options: 1) 5 moles, 2) 10 moles, 3) 1 mole, or 4) 20 moles.

Solution

To solve this problem, we need to use the concept of stoichiometry and the given thermochemical equation. The stoichiometry of a chemical equation relates the number of moles of reactants and products.

From the given equation, we can see that 2 moles of SO2 react with 1 mole of O2 to produce 2 moles of SO3. The stoichiometric ratio is 2:1:2.

Since the reaction is exothermic (heat is released), the value of ΔH is negative (-198 kJ). This means that the reaction is releasing energy.

Now, let's calculate the amount of oxide (IV) consumed using the given information.

We know that 1980 kJ of heat is released during the reaction. This is the value of ΔH. We can set up a proportion to relate the heat released to the moles of oxide (IV) consumed.

Using the stoichiometric ratio, we can write the proportion as:

198 kJ / 2 moles = 1980 kJ / x moles

Simplifying the proportion:

198 / 2 = 1980 / x

99 = 1980 / x

Cross-multiplying:

99x = 1980

x = 1980 / 99

x ≈ 20

Therefore, the amount of oxide (IV) consumed is approximately 20 moles. So, the correct option is 4) 20 moles.

Answer

The amount of oxide (IV) consumed in the reaction is approximately 20 moles.