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boyakko [2]
3 years ago
11

7) All of the following are

Chemistry
1 answer:
Nat2105 [25]3 years ago
5 0

Answer:

D. Oxygen

Explanation:

External factors of photosynthesis

  • Light intensity
  • Temperature
  • Chlorophyll content
  • Carbon dioxide

Immediate product

  • Glucose

Byproduct

  • <em>Oxygen</em>

Hope this helps ;) ❤❤❤

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Suppose hydrochloric acid reacts with potassium sulfite yielding water, sulfur dioxide, and potassium chloride. Suppose 4 moles
anzhelika [568]

Answer:

128 grams of sulfur dioxide are produced.

Explanation:

2HCl+K_2SO_3\rightarrow SO_2+2KCl+H_2O

Moles of HCl = 4 moles

According to reaction, 2 moles of HCl gives 1 mole of sulfur dioxide gas.

Then 4 moles of HCl will give:

\frac{1}{2}\times 4 moles=2 moles of sulfur dioxide gas.

Mass of sulfur dioxide gas = 2 mol × 64 g/mol = 128 g

128 grams of sulfur dioxide are produced.

4 0
3 years ago
Aerosol cans contain a written warning not to subject the can to high temperatures or incinerate. Suppose an aerosol can is heat
Zanzabum
D. there would be a proportional increase in pressure to temperature
8 0
3 years ago
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What is the relative atomic mass of an element
Gennadij [26K]

Answer:

20.2 amu.

Explanation:

Let A represent isotope ²⁰X

Let B represent isotope ²²X

From the question given above, the following data were obtained:

For Isotope A (²⁰X):

Mass of A = 20

Abundance (A%) = 90%

For Isotope B (²²X):

Mass of B = 22

Abundance (A%) = 10%

Relative atomic mass (RAM) =?

The relative atomic mass (RAM) of the element can be obtained as follow:

RAM = [(Mass of A × A%)/100] + [(Mass of B × B%)/100]

RAM = [(20 × 90)/100] + [(22 × 10)/100]

RAM = 18 + 2.2

RAM = 20.2 amu

Thus, relative atomic mass (RAM) of the element is 20.2 amu

4 0
2 years ago
During photosynthesis plants take in light energy from the sun carbon dioxide from the air and water to the roots which of the f
Genrish500 [490]

Glucose sugar and oxygen

5 0
3 years ago
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A student dissolves 15.0 g of ammonium chloride(NH4Cl) in 250. 0 g of water in a well-insulated open cup. She then observes the
iren2701 [21]

Answer:  

1) Endothermic.  

2) Q_{rxn}=4435.04J  

3) \Delta _rH=15.8kJ/mol

Explanation:  

Hello there!  

1) In this case, for these calorimetry problems, we can realize that since the temperature decreases the reaction is endothermic because it is absorbing heat from the solution, that is why the temperature goes from 22.00 °C to 16.0°C.  

2) Now, for the total heat released by the reaction, we first need to assume that all of it is released by the solution since it is possible to assume that the calorimeter is perfectly isolated. In such a way, it is also valid to assume that the specific heat of the solution is 4.184 J/(g°C) as it is mostly water, therefore, the heat released by the reaction is:

Q_{rxn}=-(15.0g+250.0g)*4.184\frac{J}{g\°C}(16.0-20.0)\°C\\\\ Q_{rxn}=4435.04J    

3) Finally, since the enthalpy of reaction is calculated by dividing the heat released by the reaction over the moles of the solute, in this case NH4Cl, we proceed as follows:

\Delta _rH=\frac{ Q_{rxn}}{n}\\\\\Delta _rH= \frac{ 4435.04J}{15.0g*\frac{1mol}{53.49g} } *\frac{1kJ}{1000J} \\\\\Delta _rH=15.8kJ/mol

Best regards!  

Best regards!

4 0
3 years ago
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