Nitrogen dioxide, a major air pollutant, can be produced by the combustion of nitrogen oxide as shown.

2 answers:

8 0

Percent yield is calculated by obtaining the ratio of the actual yield and the theoretical yield times 100.

Actual yield = 1500 kg

Theoretical yield = 1500 ( 1 / 30.00 ) ( 2 / 2 ) ( 46.006 / 1 ) = 2300.3 kg

Percent yield = 1500 / <span>2300.3</span> x 100 =<span> 65.21 %

Therefore, the correct answer is the last option. Hope this answers the question.</span>

xxTIMURxx [149]3 years ago

8 0

Answer is: the percent yield is 65.2%.

Balanced chemical reaction: 2NO + O₂ → 2NO₂.

m(NO) = 1500 kg; mass of nitrog oxide.

From balanced chemical reaction: n(NO) : n(NO₂) = 2 : 2 (1 : 1).

m(NO) : M(NO) = m(NO₂) : M(NO₂).

1500 kg : 30 g/mol = m(NO₂) : 46 g/mol.

m(NO₂) = 1500 kg · 46 g/mol ÷ 30 g/mol.

m(NO₂) = 2300 kg.

the percent yield = 1500 kg ÷ 2300 kg · 100%.

the percent yield = 65.21%.

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Rus_ich [418]

Answer:

$\Delta\text{H}_1+2\Delta\text{H}_2-\Delta\text{H}_3$

Explanation:

Hess's Law of Constant Heat Summation states that if a chemical equation can be written as the sum of several other chemical equations, the enthalpy change of the first chemical equation is equal to the sum of the enthalpy changes of the other chemical equations. Thus, the reaction that involves the conversion of reactant A to B, for example, has the same enthalpy change even if you convert A to C, before converting it to B. Regardless of how many steps it takes for the reactant to be converted to the product, the enthalpy change of the overall reaction is constant.

With Hess's Law in mind, let's see how A can be converted to 2C +E.

$\bf{\text{A} \rightarrow 2\text{B}}$ (Δ $\text{H}_1$ ) -----(1)

Since we have 2B, multiply the whole of II. by 2:

$\bf{2\text{B} \rightarrow 2\text{C} +2\text{D}}$ (2Δ $\text{H}_2$ ) -----(2)

This step converts all the B intermediates to 2C +2D. This means that the overall reaction at this stage is $\text{A} \rightarrow 2\text{C} +2\text{D}$ .

Reversing III. gives us a negative enthalpy change as such:

$\bf{2\text{D} \rightarrow \text{E}}$ (-Δ $\text{H}_3$ ) -----(3)

This step converts all the D intermediates formed from step (2) to E. This results in the overall equation of $\text{A} \rightarrow 2\text{C} +\text{E}$ , which is also the equation of interest.