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3 years ago

Based on the diagram below, rank the three objects from least dense to most dense.

1 answer:

3 0

We are not given the diagram needed for this question so it would be better to talk about how to determine which object would be the most dense and least dense. One way to determine this is by looking at the densities of these objects. Higher value means the most dense while the lower value is the opposite.

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What explanation accounts for the observation that the mass of the products in reaction #1 (open system) were not equal?

Anna007 [38]

Answer:

The law of conservation of mass states that matter can not be created or destroyed in a chemical reaction.

Explanation:

5 0

2 years ago

Given the formula: what is a chemical name of this compound? propane propanal propanol propanone

katrin [286]

1) Chemical formula for propane is CH₃-CH₂-CH₃.
Propane is a three carbon alkane (acyclic saturated hydrocarbon).
2) Chemical formula for propanal is CH₃-CH₂-CH=O.
Propanal is a saturated three carbon aldehyde (have a carbonyl center).
3) Chemical formula for propanol is CH₃-CH₂-CH₂-OH.
1-propanol is a primary alcohol.
4) Chemical formula for propanone is (CH₃)₂-C=O.
Propanone or acetone is he simplest and smallest ketone.

7 0

3 years ago

A sample of 53.0 of carbon dioxide was obtained by heating 1.31 g of calcium carbont. What is the percent yield for this reactio

MaRussiya [10]

Answer:

92.04%

Explanation:

Given:

Mass of CO₂ obtained = 53.0 grams

Mass of calcium carbonate heated = 1.31 grams

Now,

the molar mass of the calcium carbonate = 100.08 grams

The number of moles heated in the problem = Mass / Molar mass

= (1.31 grams) / (100.08 grams/moles)

= 0.013088 moles

now,

1 mol of calcium carbonate yields 1 mol of CO₂

thus,

0.013088 moles of calcium carbonate will yield = 0.013088 mol of CO₂

now,

Theoretical mass of 0.013088 moles of CO₂ will be

= Number of moles × Molar mass of CO₂

= 0.013088 × 44 = 0.5758 grams

Thus, the percent yield for this reaction = $\frac{\textup{Actual yield}}{\textup{Theoretical yield}}\times100$

the percent yield for this reaction = $\frac{0.53}{0.5758}\times100$

the percent yield for this reaction = 92.04%

6 0

3 years ago

A chemist prepares a solution of silver(I) nitrate by measuring out of silver(I) nitrate into a volumetric flask and filling the

leva [86]

Answer:

3.33 M

Explanation:

It seems your question is incomplete, however, that same fragment has been found somewhere else in the web:

" A chemist prepares a solution of silver nitrate (AgNO3) by measuring out 85.g of silver nitrate into a 150.mL volumetric flask and filling the flask to the mark with water.

Calculate the concentration in mol/L of the chemist's silver nitrate solution. Be sure your answer has the correct number of significant digits. "

In this case, first we calculate the moles of AgNO₃, using its molecular weight:

85.0 g AgNO₃ ÷ 169.87 g/mol = 0.500 mol AgNO₃

Then we convert the 150 mL of the volumetric flask into L:

150 / 1000 = 0.150 L

Finally we divide the moles by the volume:

0.500 mol AgNO₃ / 0.150 L = 3.33 M

4 0

2 years ago

Write a balanced equation for each of these chemical reactions potassium phosphate + calcium nitrate

cupoosta [38]

It forms calcium phosphate and potassium nitrate
2 K3PO4 + 3Ca(NO3)2 --> Ca3(PO4)2 + 6KNO3

7 0

3 years ago