A gas occupies 900.0 mL at a temperature of 27.0 . What is the volume at 132.0 °C?

Answers

Answer 1

Answer: V₁ = 900.0 mL

T₁ = 27.0ºC + 273 = 300 K

V₂ = ?

T₂ = 132.0 + 273 = 405 K

V₁ / T₁ = V₂ / T₂

900.0 / 300 = V₂ / 405

300 x V₂ = 405 x 900.0

300 x V₂ = 364500

V₂ = 364500 / 300

V₂ = 1215 mL

hope this helps!

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How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol.4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

Answers

First, convert the amount of KNO3 to moles using the molar mass:
58.6 g / 101.11 g/mol = 0.5796 mol KNO3

Next, using the given balanced reaction, use the stoichoimetric ratio to calculate the number of mole of oxygen that will be produced. From the reaction, for every 4 moles of KNO3 that decomposes, there are 5 moles of O2 formed. So,
0.5796 mol KNO3 x (5/4) = 0.7254 moles O2

Therefore, when 58.6 g of KNO3 decomposes, there are 0.7254 moles of O2 that will be formed.

The moles of oxygen formed when 58.6 g of KNO3 decomposes is $\boxed{{\text{0}}{\text{.7245moles}}}$

Further Explanation:

Stoichiometry of a reaction is used to determine the amount of species present in the reaction by the relationship between the reactants and products. It can be used to determine the moles of a chemical species when the moles of other chemical species present in the reaction is given.

Consider the general reaction,

${\text{A}}+2{\text{B}}\to3{\text{C}}$

Here,

A and B are reactants.

C is the product.

One mole of A reacts with two moles of B to produce three moles of C. The stoichiometric ratio between A and B is 1:2, the stoichiometric ratio between A and C is 1:3 and the stoichiometric ratio between B and C is 2:3.

The given reaction is,

${\text{4KN}}{{\text{O}}_3}\left(s\right)\to2{{\text{K}}_2}{\text{O}}\left(s\right)+2{{\text{N}}_2}\left(g\right)+5{{\text{O}}_2}\left(g\right)$

 On reactant side,

Number of potassium atoms is 4.

Number of nitrogen atom is 4.

Number of oxygen atoms is 12.

 On the product side,

Number of potassium atoms is 4.

Number of nitrogen atom is 4.

Number of oxygen atoms is 12.

The number of atoms of all the species in both the reactant and the product side is the same. So above reaction is balanced. The stoichiometry of the balanced reaction indicates that 4 moles of ${\text{KN}}{{\text{O}}_3}$ decompose to give 2 moles of ${{\text{K}}_2}{\text{O}}$ to form 2 moles of ${{\text{N}}_2}$ and 5 moles of ${{\text{O}}_2}$ .

The formula to calculate the number of moles of ${\mathbf{KN}}{{\mathbf{O}}_{\mathbf{3}}}$ is as follows:

${\text{Moles of KN}}{{\text{O}}_3}=\frac{{{\text{Given mass of KN}}{{\text{O}}_3}}}{{{\text{Molar mass of KN}}{{\text{O}}_3}}}$ …… (1)

The given mass of is 58.6 g.

The molar mass of is 101.11 g/mol.

Substitute these values in equation (1)

$\begin{gathered}{\text{Moles of KN}}{{\text{O}}_3}{\mathbf{=}}\left({58.6\;{\text{g}}}\right)\left({\frac{{{\text{1}}\;{\text{mol}}}}{{{\text{101}}{\text{.11}}\;{\text{g}}}}}\right)\n=0.5796\;{\text{mol}}\n\end{gathered}$

According to the stoichiometry, 4 moles of ${\text{KN}}{{\text{O}}_3}$ decompose to give 2 moles of ${{\text{K}}_2}{\text{O}}$ , 2 moles of {{\text{N}}_2} and 5 moles of ${{\text{O}}_2}$ .

So the number of moles of {{\mathbf{O}}_{\mathbf{2}}} formed by 0.5796 moles of ${\mathbf{KN}}{{\mathbf{O}}_{\mathbf{3}}}$ is calculated as follows:

$\begin{gathered}{\text{Moles of }}{{\text{O}}_2}{\mathbf{=}}\left({\frac{{5\;{\text{mol}}}}{{4\;{\text{mol}}}}}\right)*\left({0.5796\;{\text{mol}}}\right)\n=0.7245\;{\text{mol}}\n\end{gathered}$

Hence, the moles of ${{\mathbf{O}}_{\mathbf{2}}}$ produced is 0.7245 moles.

Learn more:

1. Bond energy of H-H bond in the given reaction: brainly.com/question/7213980

2. What coefficients are required to balance equation: brainly.com/question/1971314

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Mole concept

Keywords: stoichiometry, KNO3, K2O, O2, N2, moles, A, B, C, molar mass, reactants, products, 0.5796 moles, 0.7245 moles, potassium, oxygen and nitrogen.

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Answers

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an organic compound on analysis yielded 2.04g carbon, 0.34g hydrogen, 2.73g oxygen. calculate the empirical formula

Answers

Answer:

CH2O

Explanation:

According to this question:

C = 2.04g

H = 0.34g

O = 2.73g

First, we divide the mass value of each element by its atomic mass to convert to moles.

C = 2.04g ÷ 12 = 0.17mol

H = 0.34g ÷ 1 = 0.34mol

O = 2.73g ÷ 16 = 0.17mol

Next, we divide by the smallest mole value (0.17):

C = 0.17mol = 0.17 = 1

H = 0.34mol ÷ 0.17 = 2

O = 0.17mol ÷ 0.17 = 1

The whole number ratio of C,H,O is 1:2:1, hence, the empirical formula is CH2O.

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Answers

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Which of the following is a chemical property of vinegar? A. The pH of vinegar is around 2.4. B. Vinegar freezes at around 2°C. C. Vinegar boils at about 100°C. D. The color of vinegar ranges from colorless to brown. E. Vinegar is a transparent liquid.

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I think the correct answer from the choices listed above is option A. The chemical property of a vinegar is that the pH of vinegar is around 2.4. It tells something about the concentration of hydrogen ions in the solution. The other choices given only describe the physical properties of the substance.

Answer:

Explanation:

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