Answer:
Chalcogen
Explanation:
The table below shows properties of two compounds at standard pressure. Which statement classifies the two compounds? 1)Both compounds are ionic, 2)Both compounds are molecular, 3) Compound 1 is ionic, and compound 2 is molecular, 4)Compound 1 is molecular, and compound is ionic
Answer:
answer of this question is option. 3. compound 1 is ionic ,and 2 is molecular
Compound 1 is ionic and compound 2 is molecular. The correct option is 3) Compound 1 is ionic, and compound 2 is molecular
From the question,
We are to classify the compounds according to the information provided in the table
First,
We will list the properties of ionic and molecular compounds
Properties of ionic compounds
The exist as solid at room temperature. They generally have high melting and boiling temperatures. They are good electrical conductors when molten or in solution.Properties of molecular compounds
They can exist as solid, liquid or gas.They generally have low melting and boiling temperatures. They are poor electrical conductors.In the given table,
Compound 1 has high melting and boiling points, and it is a good electrical conductor. Therefore, compound 1 is ionic
Compound 2 has low melting and boiling points, and it is a poor electrical conductor. Therefore, compound 2 is molecular
Hence, Compound 1 is ionic and compound 2 is molecular. The correct option is 3) Compound 1 is ionic, and compound 2 is molecular
Learn more on properties of ionic and molecular compounds here: https://brainly.com/question/13878434
what is the mass in grams of 0.40 moles of sodium borohydride nabh4
Answer:
15.12g
Explanation:
Given parameters:
Number of moles = 0.4moles
Unknown:
Mass of the compound = ?
Solution:
To solve this problem;
Mass = number of moles x molar mass
Molar mass of NaBH₄ = 23 + 10.8 + 4(1) = 37.8g/mol
Mass of the compound = 0.4 x 37.8 = 15.12g
Answer:
The answer is 15.12 g but if you are taking this test on ck12 make sure you round it to 15 like it says on the directions :) good luck
atom ,molecule, proton neutron electron, elements/compounds from SMALLEST to the BIGGEST.
Answer:
Electron,Protons/Neutrons,Atom,Molecule
Explanation:
A 0.4647-g sample of a compound known to contain only carbon, hydrogen, and oxygen was burned in oxygen to yield 0.8635 g of CO2 and 0.1767 g of H2O. What is the empirical formula of the compound?
Answer: The empirical formula is [tex]C_3H_3O_2[/tex].
Explanation:
The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:
[tex]C_xH_yO_z+O_2\rightarrow CO_2+H_2O[/tex]
where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.
We are given:
Mass of [tex]CO_2[/tex] = 0.8635
Mass of [tex]H_2O[/tex]= 0.1767 g
Molar mass of carbon dioxide = 44 g/mol
Molar mass of water = 18 g/mol
For calculating the mass of carbon:
In 44g of carbon dioxide, 12 g of carbon is contained.
So, in 0.8635 g of carbon dioxide, =[tex]\frac{12}{44}\times 0.8635=0.2355g[/tex] of carbon will be contained.
For calculating the mass of hydrogen:
In 18g of water, 2 g of hydrogen is contained.
So, in 0.1767 g of water, =[tex]\frac{2}{18}\times 0.1767=0.0196g[/tex] of hydrogen will be contained.
Mass of oxygen in the compound = (0.4647) - (0.2355+0.0196) = 0.2096 g
Mass of C = 0.2355 g
Mass of H = 0.0196 g
Step 1 : convert given masses into moles.
Moles of C =[tex] \frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{0.2355g}{12g/mole}=0.0196moles[/tex]
Moles of H=[tex]\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.0196g}{1g/mole}=0.0196moles[/tex]
Moles of O=[tex]\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{0.2096g}{16g/mole}=0.0131moles[/tex]
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For C =[tex]\frac{0.0196}{0.0131}=1.5[/tex]
For H =[tex]\frac{0.0196}{0.0131}=1.5[/tex]
For O = [tex]\frac{0.0131}{0.0131}=1[/tex]
The ratio of C : H: O = 1.5 : 1 .5 : 1
Converting to simple whole number ratio:
The ratio of C : H: O = 3 : 3: 2
Hence the empirical formula is [tex]C_3H_3O_2[/tex].
which mineral is composed of calcium and fluorine?
Answer:
Fluorite
What is Fluorite? Fluorite is an important industrial mineral composed of calcium and fluorine (CaF2). It is used in a wide variety of chemical, metallurgical, and ceramic processes
A student working in the laboratory produces 6.81 grams of calcium oxide, CaO, from 20.7 grams of calcium
carbonate, CaCO3, according to the reaction CaCO3 → CaO + CO2. Calculate the theoretical yield and
the percent yield for the reaction. Show and/or explain your work.
Answer:
A. Theoretical yield of CaO is 11.59 g
B. Percentage yield of CaO = 58.76%
Explanation:
The following data were obtained from the question:
Mass of CaCO₃ = 20.7 g
Actual yield of CaO = 6.81 g
Theoretical yield of CaO =?
Percentage yield of CaO =?
The equation for the reaction is given below:
CaCO₃ —> CaO + CO₂
Next, we shall determine the mass of CaCO₃ that decomposed and the mass of CaO produced from the balanced equation. This can be obtained as follow:
Molar mass of CaCO₃ = 40 + 12 + (3×16)
= 40 + 12 + 48
= 100 g/mol
Mass of CaCO₃ from the balanced equation = 1 × 100 = 100 g
Molar mass of CaO = 40 + 16 = 56 g/mol
Mass of CaO from the balanced equation = 1 × 56 = 56 g
SUMMARY:
From the balanced equation above,
100 g of CaCO₃ decomposed to produce 56 g of CaO.
A. Determination of the theoretical yield of CaO.
From the balanced equation above,
100 g of CaCO₃ decomposed to produce 56 g of CaO.
Therefore, 20.7 g of CaCO₃ will decompose to produce =
(20.7 × 56)/100 = 11.59 g of CaO.
Thus, the theoretical yield of CaO is 11.59 g
B. Determination of the percentage yield.
Actual yield of CaO = 6.81 g
Theoretical yield of CaO = 11.59 g
Percentage yield of CaO =?
Percentage yield = Actual yield /Theoretical yield × 100
Percentage yield = 6.81/11.59 × 100
Percentage yield of CaO = 58.76%
BRAINLLEST! Boiling water for mac and cheese is a physical change. Give 2 pieces of evidence to support this claim
Answer:
In explanation.
Explanation:
Physical changes are generally changes in states of matter. So, the water going from liquid to gas is a phase change and therefore physical. (It's still water, just in a different form). Im not sure about the second piece of evidence though. Unless you are talking about the Mac and Cheese which in that case is also a physical change as the two ingredients cheese and macaroni stay the same when cooked just become softer and edible.