A 1.775g sample mixture of KHCO₃ is decomposed by heating. if the mass loss is 0.275g, the mass percentage of KHCO₃ is 70.4%.
<h3>What is a decomposition reaction?</h3>
A decomposition reaction can be defined as a chemical reaction in which one reactant breaks down into two or more products.
- Step 1: Write the balanced equation for the decomposition of KHCO₃.
2 KHCO₃(s) → K₂CO₃(s) + CO₂(g) + H₂O(l)
The mass loss of 0.275 g is due to the gaseous CO₂ that escapes the sample.
- Step 2: Calculate the mass of KHCO₃ that formed 0.275 g of CO₂.
In the balanced equation, the mass ratio of KHCO₃ to CO₂ is 200.24:44.01.
0.275 g CO₂ × 200.24 g KHCO₃/44.01 g CO₂ = 1.25 g KHCO₃
- Step 3: Calculate the mass percentage of KHCO₃ in the sample.
There are 1.25 g of KHCO₃ in the 1.775 g sample.
%KHCO₃ = 1.25 g/1.775 g × 100% = 70.4%
A 1.775g sample mixture of KHCO₃ is decomposed by heating. if the mass loss is 0.275g, the mass percentage of KHCO₃ is 70.4%.
Learn more about decomposition reactions here: brainly.com/question/14219426
The number of mole of oxygen needed is of 0.080 mole.
To solve this question, we'll begin by writing the balanced equation for the reaction. This is illustrated below:
<h3>CH₃COOH + 2O₂ —> CO₂ + 2H₂O</h3>
From the balanced equation above,
2 moles of O₂ reacted to produce 2 moles of H₂O.
Finally, we shall determine the number of mole of O₂ needed to produce 0.080 mole of H₂O. This can be obtained as follow:
From the balanced equation above,
2 moles of O₂ reacted to produce 2 moles of H₂O.
Therefore,
0.080 mole of O₂ will also react to produce 0.080 mole of H₂O.
Thus, 0.080 mole of oxygen, O₂, is needed for the reaction.
Learn more: brainly.com/question/1563415
It can be easily judged that only the first reaction is an acid base reaction among the three given in the question. So, we can avoid the other two reactions given in the question. Now let us focus and write down the balanced chemical equation of <span>P-Toluidine + HCl.
</span><span>C7H9N + HCl = C7H10N (+) + Cl (-)
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I hope the answer has come to your help.
