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Talja [164]
3 years ago
14

The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 17

75. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide () into liquid mercury and gaseous dioxygen. 2. Suppose if dioxygen gas are produced by this reaction, at a temperature of and pressure of exactly . Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
pantera1 [17]3 years ago
4 0

Answer:

1. HgO(s) → Hg(l) + 0.5 O₂(g)

2. 0.858 g

Explanation:

There is some info missing. I think this is the original question.

<em>The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. </em>

<em>1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. </em>

<em>2. Suppose 59.0 mL of dioxygen gas are produced by this reaction, at a temperature of 90.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.</em>

<em />

1.

The balanced chemical equation is:

HgO(s) → Hg(l) + 0.5 O₂(g)

2.

First, we will calculate the moles of O₂ using the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 1 atm × 0.0590 L / 0.0821 atm.L/mol.K × 363.2 K

n = 1.98 × 10⁻³ mol

The molar ratio of HgO to O₂ is 1:0.5. The moles of HgO are (1/0.5) × 1.98 × 10⁻³ mol = 3.96 × 10⁻³ mol

The molar mass of HgO is 216.59 g/mol. The mass of HgO is:

3.96 × 10⁻³ mol × 216.59 g/mol = 0.858 g

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I NEED HELP PLEASE!!!! CHEMISTRY QUESTION: If 38 g of Li3P and 15 grams of Al2O3 are reacted, what total mass of products will r
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Answer:

21.5 g.

Explanation:

Hello!

In this case, since the reaction between the given compounds is:

2Li_3P+Al_2O_3\rightarrow 3Li_2O+2AlP

We can see that according to the law of conservation of mass, which states that matter is neither created nor destroyed during a chemical reaction, the total mass of products equals the total mass of reactants based on the stoichiometric proportions; in such a way, we first need to compute the reacted moles of Li3P as shown below:

n_{Li_3P}^{reacted}=38gLi_3P*\frac{1molLi_3P}{51.8gLi_3P}=0.73molLi_3P

Now, the moles of Li3P consumed by 15 g of Al2O3:

n_{Li_3P}^{consumed \ by \ Al_2O_3}=15gAl_2O_3*\frac{1molAl_2O_3}{101.96gAl_2O_3} *\frac{2molLi_3P}{1molAl_2O_3} =0.29molLi_3P

Thus, we infer that just 0.29 moles of 0.73 react to form products; which means that the mass of formed products is:

m_{Li_2O}=0.29molLi_3P*\frac{3molLi_2O}{2molLi_3P} *\frac{29.88gLi_2O}{1molLi_2O} =13gLi_2O\\\\m_{AlP}=0.29molLi_3P*\frac{2molAlP}{2molLi_3P} *\frac{57.95gAlP}{1molAlP} =8.5gAlP

Therefore, the total mass of products is:

m_{products}=13g+8.5g\\\\m_{products}=21.5g

Which is not the same to the reactants (53 g) because there is an excess of Li₃P.

Best Regards!

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