Chemistry: How much energy is needed to raise the temperature of 850g of aluminum from 22.8 °C to 194.66 if the specific heat of aluminum

Percentage yield of carbonic acid: 88%.Explanation:Balance the equation:.Relative atomic mass data from a modern periodic table:Na: 22.990;H: 1.008;C: 12.011;O: 15.999.Formula mass:NaHCO₃: .H₂CO₃: .Number of moles of NaHCO₃ in the sample:.How many moles of carbonic acid will that many NaHCO₃ produce in theory? The ratio between the coefficient in front of NaHCO₃ and H₂CO₃ in the balanced equation is 2:1. In other words, it takes two moles of NaHCO₃ to produce one mole of H₂CO₃. In other words, 0.0385687...

How much energy is needed to raise the temperature

Ответ:

heavendavis101

11.11.2022

Chemistry

Percentage yield of carbonic acid: 88%.

Explanation:

Balance the equation:

${\bf 2}\;\text{NaHCO}_3 \to \text{Na}_2\text{CO}_3 + \text{H}_2\text{CO}_3$ .

Relative atomic mass data from a modern periodic table:

Na: 22.990;H: 1.008;C: 12.011;O: 15.999.

Formula mass:

NaHCO₃: $22.990 + 1.008 + 12.011 + 3\times 15.999=84.006\;\text{g}\cdot\text{mol}^{-1}$ .H₂CO₃: $2\times 1.008+ 12.011 + 15.999 = 62.024\;\text{g}\cdot\text{mol}^{-1}$ .

Number of moles of NaHCO₃ in the sample:

$\displaystyle n(\text{NaHCO}_3)= \frac{m}{M} = \frac{3.24}{84.006} = 0.0385687\;\text{mol}$ .

How many moles of carbonic acid will that many NaHCO₃ produce in theory? The ratio between the coefficient in front of NaHCO₃ and H₂CO₃ in the balanced equation is 2:1. In other words, it takes two moles of NaHCO₃ to produce one mole of H₂CO₃.

$\displaystyle n(\text{H}_2\text{CO}_3) = \frac{1}{2}\;n(\text{NaHCO}_3) = \frac{1}{2} \times 0.0385687 = 0.0192843\;\text{mol}$

In other words, 0.0385687 moles of NaHCO₃ will produce 0.0192843 moles of H₂CO₃.

What will be the theoretical yield of H₂CO₃?

$m(\text{H}_2\text{CO}_3,\;\text{theoretical}) = n\cdot M = 0.0192843\times 62.024 = 1.19609\;\text{g}$ .

What's the actual yield of H₂CO₃?

Mass conserves. As a result, the difference between the mass of the solid before and after the reaction is the mass of the H₂O and CO₂ that escaped. The two species combine to form H₂CO₃. The mass of the H₂CO₃ produced will be the same as the change in the mass of the solid.

$m(\text{H}_2\text{CO}_3,\;\text{actual}) = m(\text{solid},\;\text{initial}) - m(\text{solid},\;\text{final})= 3.24 - 2.19 = 1.05\;\text{g}$ .

What's the percentage yield of H₂CO₃?

$\displaystyle \begin{aligned}\text{Percentage Yield} &= \frac{\text{Actual Yield}}{\text{Theoretical Yield}}\times 100\% \\&= \frac{1.05}{1.19609}\times 100\%\\&=87.8\%\end{aligned}$ .

Note: all values in this question are in 3 sig. fig. Keep more than 3 sig. fig. in the calculations but round the final result to 3 sig. fig.

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How much energy is needed to raise the temperature of 850g of aluminum from 22.8 °C to 194.66 if the specific heat of aluminum

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