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3 years ago

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A piece of metal that has a density of 5.2 g/cm3 and a mass of 100 g was placed in a full jar of water. How many mL of water was

spilled out of the jar? Note: one cm^3 = one mL

1 answer:

Klio2033 [76]3 years ago

5 0

Answer:

100g / (5.2g/cm3)

= 100g / (5.2g / 1cm3)

= 100g x 1cm3 / 5.2 g

= 19.2 cm3

Since 1 cm3 = 1 ml, your answer is 19.2 ml.

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Which substance is the reducing agent in this reaction? 16h++2cr2o72−+c2h5oh→4cr3++11h2o+2co2 express your answer as a chemical

lana66690 [7]

16 H + + 2Cr2O72- + C2H5OH → 4 Cr3 + +11H2O +2CO2

The reducing agent is C2H5OH

Explanation

reducing agent is a substance that loses or donate electrons in a chemical reaction. C2H5OH is the one which donate electrons in the above chemical equation.

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Acetylene gas (c2h2) reacts with oxygen gas (o2) to produce carbon dioxide (co2) and water vapor (h2o). how many liters of c2h2

MissTica

According to the balanced equation of the reaction:

2C2H2 + 5O2 → 4CO2 + 2H2O

So we can mention all as liters,

A) as we see that 2 liters of C2H2 react with 5 liters of oxygen to produce 4 liters of CO4 and 2 liters of H2O

So, when we have 75L of CO2

and when we have 2 L of C2H2 reacts and gives 4 L of CO2

2C2H2 → 4CO2

∴ The volume of C2H2 required is:

= 75L / 2

= 37.5 L

B) and, when we have 75 L of CO2

and 4CO2 → 2H2O

∴ the volume of H2O required is:

= 75 L /2
= 37.5 L

C) and from the balanced equation and by the same way:

when 5 liters O2 reacts to give 4 liters of CO2

and we have 75 L of CO2:

5 O2 → 4 CO2

?? ← 75 L

∴ the volume of O2 required is:

= 75 *(5/4)

= 93.75 L

D) about the using of the number of moles the answer is:

no, there is no need to find the number of moles as we called everything in the balanced equation by liters and use it as a liter unit to get the volume, without the need to get the number of moles.

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3 years ago

Read 2 more answers

This is the question i need help on

mash [69]

I thank that your answer is C.

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4 years ago

A 2.912 g sample of a compounds containing only C, H, and O was completely oxidized in a reaction that yielded 3.123 g of water

Taya2010 [7]

Answer:

Explanation:

18 gram of water contains 2 g of hydrogen

3.123 gram of water will contain 2 x 3.123 / 18 = .347 g of hydrogen .

44 gram of carbon dioxide contains 12 g of carbon

7.691 gram of carbon dioxide will contain 12 x 7.691 / 44 = 2.1 g of carbon .

So the sample will contain 2.912 - ( .347 + 2.1 ) g of oxygen .

= .465 g of oxygen .

moles of Carbon = 2.1 / 12 = .175

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moles of oxygen = .465 / 16 = .029

Ratio of moles of carbon , oxygen and hydrogen ( C,O,H )

= 0.175 : 0.029 : 0.347

= .175/ .029 : 1 : .347 / .029

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So empirical formula = C₆H₁₂O

Let the molecular formula be $(C_6H_{12}O)_n$

molecular weight = n ( 6 x 12 + 12x 1 + 16)

= 100 n

Given 100 n = 100.1

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Molecular formula = C₆H₁₂O.

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According to observations, the overall chemical composition of our solar system and other similar star systems is approximately

jonny [76]

Answer:A

Explanation:

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Like the Sun, the mass of Jupiter and Saturn are composed of roughly 98% hydrogen and helium with 2% of all the other elements combined.

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