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larisa [96]
3 years ago
15

Which sound has waves with the greatest amplitude?'

Chemistry
1 answer:
Furkat [3]3 years ago
8 0
Jet Takeoff because it is the loudest according to the chart by the number of decibels.
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For an assignment, Alexis has to write a scientific question. She writes, "How much money should be spent to research brain canc
Andru [333]

Answer:

D will brain cancer eventually be curable?

Explanation:

3 0
4 years ago
The rate of weathering depends on?
andrezito [222]
Amount of water in air

Temperature of the area
7 0
3 years ago
The following reaction shows the products when sulfuric acid and aluminum hydroxide react.
scoray [572]

Leftover: approximately 11.73 g of sulfuric acid.

<h3>Explanation</h3>

Which reactant is <em>in excess</em>?

The theoretical yield of water from Al(OH)₃ is lower than that from H₂SO₄. As a  result,

  • Al(OH)₃ is the limiting reactant.
  • H₂SO₄ is in excess.

How many <em>moles</em> of H₂SO₄ is consumed?

Balanced equation:

2 Al(OH)₃ + 3 H₂SO₄ → Al₂(SO₄)₃ + 6 H₂O

Each mole of Al(OH)₃ corresponds to 3/2 moles of H₂SO4. The formula mass of Al(OH)₃ is 78.003 g/mol. There are 15 / 78.003 = 0.19230 moles of Al(OH)₃ in the five grams of Al(OH)₃ available. Al(OH)₃ is in excess, meaning that all 0.19230 moles will be consumed. Accordingly, 0.19230 × 3/2 = 0.28845 moles of H₂SO₄ will be consumed.

How many <em>grams</em> of H₂SO₄ is consumed?

The molar mass of H₂SO₄ is 98.076 g.mol. The mass of 0.28845 moles of H₂SO₄ is 0.28845 × 98.076 = 28.289 g.

How many <em>grams</em> of H₂SO₄ is in excess?

40 grams of sulfuric acid H₂SO₄ is available. 28.289 grams is consumed. The remaining 40 - 28.289 = 11.711 g is in excess. That's closest to the first option: 11.73 g of sulfuric acid.

6 0
3 years ago
Methane is the major component of natural gas. The standard molar enthalpy of formation of methane CH4 is -74.9 kJ/mol. For the
arlik [135]

Answer:

\Delta _rH=-802.2kJ/mol

Explanation:

Hello!

In this case, according to the given chemical reaction, it is possible to calculate the enthalpy change of the reaction via:

\Delta _rH=\Delta _fH_{CO_2}+2\Delta _fH_{H_2O}-\Delta _fH_{CH_4}

Since the enthalpy of formation of oxygen is 0. Thus, given the enthalpies of formation of gaseous carbon dioxide and water, we obtain:

\Delta _rH=(-393.5kJ/mol)+2(-241.8kJ/mol)-(-74.9kJ/mol)\\\\\Delta _rH=-802.2kJ/mol

Best regards!

3 0
3 years ago
A gas has a pressure of 0.470 atm at 60.0 C. What is the pressure at standard temperature?
OLEGan [10]

Answer:

P2=0.385atm

Explanation:

step one:

Given that the temperature T1=  60 Celcius

we can convert this to kelvin by adding 273k to 60 Celcius

we have T1= 333k

pressure P1= 0.470 atm

step two:

we know that the standard temperature is T2= 273K

Applying the temperature and pressure relationship we have

P1/T1=P2/T2

substituting our given data we have

0.47/333=P2/273

cross multiply we have

P2= (0.47*273)/333

P2= 128.31/333

P2=0.385 atm

6 0
3 years ago
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