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lord [1]
3 years ago
11

A hot metal plate at 150°C has been placed in air at room temperature. Which event would most likely take place over the next fe

w minutes? A.) Molecules in both the metal and the surrounding air will start moving at lower speeds. B.) Molecules in both the metal and the surrounding air will start moving at higher speeds. C.) The air molecules that are surrounding the metal will slow down, and the molecules in the metal will speed up. D.) The air molecules that are surrounding the metal will speed up, and the molecules in the metal will slow down.
Chemistry
1 answer:
prohojiy [21]3 years ago
5 0

Answer:

the air molecules that are surrounding the metal will speed up, and the molecules in the metal will slow down.

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Answer:

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tu sabias que existe el automovil que funciona solo con agua y hay otro que solo funciona con h2? pero lastimosamente estados un
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Question 13 unsaved the nonmetals in groups 5a, 6a, and 7a: question 13 options: lose electrons when they form ions. form ions w
frutty [35]

How does the law of conservation of mass apply  to this reaction: C2H4 + O2 → H2O + CO2?

6 0
4 years ago
Carbohydrates are polymers of what monomer?​
Leona [35]

Answer:

Yes, carbohydrates have both monomers and polymers. Monomers of carbohydrates are monosaccharides (mono- one; saccharide- sugar) which are simple sugars like glucose, fructose and galactose. Polymers of carbohydrates or polysaccharides include starch...

Explanation:

3 0
3 years ago
5.50g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 13
Nimfa-mama [501]

Answer:

The molecular formula is C8H8O2

Explanation:

Step 1: Data given

Mass of compound X = 5.50 grams

Mass of CO2 = 14.24 grams

Molar mass of CO2 = 44.01 g/mol

Mass of H2O = 2.91 grams

Molar mass H2O = 18.02 g/mol

Molar mass C = 12.01 g/mol

Molar mass O = 16.0 g/mol

Molar mass H = 1.01 g/mol

Molar mass of the compound = 136 g/mol

Step 2: Calculate moles CO2

Moles CO2 = 14.24 grams / 44.01 g/mol

Moles CO2 = 0.324 moles

Step 3: Calculate moles C

For 1 mol cO2 we have 1 mol C

For 0.324 moles CO2 we have 0.324 moles C

Step 4: Calculate mass C

Mass C = 0.324 moles * 12.01 g/mol

Mass C = 3.89 grams

Step 5: Calculate moles H2O

Moles H2O = 2.91 grams / 18.02 g/mol

Moles H2O = 0.161 moles

Step 6: Calculate moles H

For 1 mol H2O we have 2 moles H

For 0.161 moles H2O we have 2*0.161 = 0.322 moles H

Step 7: Calculate mass H

Mass H = 0.322 moles * 1.01 g/mol

Mass H = 0.325 grams

Step 8: Calculate mass O

Mass O = 5.50 grams - 3.89 grams - 0.325 grams

MAss O = 1.285 grams

Step 9: Calculate moles O

Moles O = 1.285 grams / 16.0 g/mol

Moles O = 0.0803 moles

Step 10: Calculate mol ratio

We divide by the smallest amount of moles

C: 0.324 moles / 0.0803 moles = 4

H: 0.322 moles / 0.0803 moles = 4

O: 0.0803 moles / 0.0803 moles = 1

The empirical formula is C4H4O

The molar mass of this empirical formula is 68 g/mol

Step 11: Calculate the molecular formula

We have to multiply the empirical formula by n

n = 136 g/mol / 68 g/mol

n = 2

We have to multiply the empirical formula by 2

Molecular formula = 2*(C4H4O) = C8H8O2

The molecular formula is C8H8O2

3 0
3 years ago
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