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3 years ago

Which one of the following groups of chemical compounds is composed entirely of organic compounds?

2 answers:

8 0

The correct answer is D.

In group A, CaSO4 is not organic; in group B, CaCl2 is not organic; in group C, Ca3(PO4)2 is not organic.

Hope this helps~

KengaRu [80]3 years ago

5 0

Answer;

D. C6H6, C2H5OH, C6H5CH3, and C3H5(NO3)3.

Explanation;

-Organic compound are chemical compounds in which one or more atoms of carbon are covalently linked to atoms of other elements, most commonly hydrogen, oxygen, or nitrogen, like the examples above in choice D. . Inorganic Compounds on the other hand, are compounds made from any elements except those compounds of carbon, such as CaSO4, CaCl2 and Ca3(PO4)2 in A, B and C respectively.

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The half-life of Palladium-100 is 4 days. After 12 days a sample of Palladium-100 has been reduced to a mass of 4 mg. What was t

Degger [83]

Answer : The initial mass of the sample is, 31.9 mg

Explanation :

Half-life = 4 days

First we have to calculate the rate constant, we use the formula :

$k=\frac{0.693}{t_{1/2}}$

$k=\frac{0.693}{4\text{ days}}$

$k=0.173\text{ days}^{-1}$

Now we have to calculate the initial mass of sample.

Expression for rate law for first order kinetics is given by:

$t=\frac{2.303}{k}\log\frac{a}{a-x}$

where,

k = rate constant = $0.173\text{ days}^{-1}$

t = time passed by the sample = 12 days

a = initial amount of the reactant = ?

a - x = amount left after decay process = 4 mg

Now put all the given values in above equation, we get

$12=\frac{2.303}{0.173}\log\frac{a}{4}$

$a=31.9mg$

Therefore, the initial mass of the sample is, 31.9 mg

3 0

4 years ago

Explain why chlorine is a gas while iodine is a solid yet both are halogens. Select one: a. Both iodine and chlorine differ in s

yarga [219]

Answer:

Chlorine has strong inter molecular forces than iodine

Explanation:

3 0

4 years ago

Read 2 more answers

To convert liters of CO2 to moles of CO2, what conversion factor would it be?

MArishka [77]

22.4L.

This is because the standard conversion factor for Liters is 22.4 and in the question it explicitly states liters of CO2.

Therefore, in order to convert Liters of CO2 to Moles of CO2, you'd need to use the conversion factor of 22.4.

Hope this helps!

3 0

3 years ago

When adjusted for any changes in δh and δs with temperature, the standard free energy change δg∘t at 2400 k is equal to 1.22×105

rosijanka [135]

When adjusted for any changes in δh and δs with temperature, the standard free energy change δg∘t at 2400 k is equal to 1.22×105j/mol, then the equilibrium constant at 2400 k is 2.21×10−3. The answer to the statement is 2.21×10−3.

6 0

3 years ago

Read 2 more answers

16.0 grams of oxygen gas reacted with 80.0 grams nitrogen monoxide gas producing 25.0 grams of nitrogen dioxide gas in the lab.

Anon25 [30]

Answer:

Limiting reactant = O₂

Excess reactant = NO

Theoretical yield of NO₂ = 46 g

Mass of excess reactant = 30 g

<h3 />

Explanation:

O₂ + 2NO → 2NO₂

Mole ratio for the reaction is;

1 : 2 → 2

mass of O₂ = 16 g

mass of NO = 80 g

mass of NO₂ = 25 g

molecular weight of O₂ = 32 g/mol

molecular weight of NO = 30 g/mol

molecular weight of NO₂ = 46 g/mol

molar mass of O₂ = mass ÷ molecular weight = 16 g ÷ 32 g/mol = 0.5 mol

molar mass of NO = mass ÷ molecular weight = 80 g ÷ 30 g/mol = 2.67 mol

Since, 1 mole of O₂ requires 2 moles of NO for the combustion reaction, 0.5 mole shall require 1 mole of NO for the reaction. Thus, O₂ is the limiting reactant and NO is the excess reactant as it has an excess of 2.67 mol - 1 mol = 1.67 mol.

<h3>Theoretical yield of NO₂</h3><h3 />

1 mole of O₂ shall yield 2 moles of NO₂

Thus, 0.5 mole of O₂ shall yield 1 mole of NO₂

mass of NO₂ = molecular weight * molar mass = 46 g/mol * 1 mole = 46 g

<h3>Mass of Excess Reactant</h3>

1 mole of O₂ shall react with 2 moles of NO

Thus, 0.5 mole of O₂ shall yield 1 mole of NO

mass of NO = molecular weight * molar mass = 30 g/mol * 1 mole = 30 g

5 0

3 years ago