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dsp73
3 years ago
11

When nonmetals react with nonemtalss, the atoms of the nonmetals?

Chemistry
1 answer:
Thepotemich [5.8K]3 years ago
4 0
Is this worded correctly?
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How many different d orbits are within the 3d sublevel
ohaa [14]

Answer:

Its 5

Explanation:

6 0
3 years ago
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During photosynthesis, how many moles of water (H₂O) are needed to produce 150 grams of glucose
Nuetrik [128]

During photosynthesis, 5 moles of water are needed to produce 150 grams of glucose. The correct option is D.

<h3>What is photosynthesis?</h3>

It is the process by which green plants and some other organisms use sunlight to synthesize nutrients from carbon dioxide and water.

  • Step 1: Write the balanced equation for photosynthesis.

6 CO₂ + 6 H₂O ⇒ C₆H₁₂O₆ + 6 O₂

  • Step 2: Convert 150 g of C₆H₁₂O₆ to moles.

The molar mass of C₆H₁₂O₆ is 180.16 g/mol.

150 g × 1 mol/180.16 g = 0.833 mol

  • Step 3: Calculate the moles of water required to form 0.833 moles of C₆H₁₂O₆

The molar ratio of H₂O to C₆H₁₂O₆ is 6:1.

0.833 mol C₆H₁₂O₆ × 6 mol H₂O/1 mol C₆H₁₂O₆ = 5.00 mol H₂O

During photosynthesis, 5 moles of water are needed to produce 150 grams of glucose. The correct option is D.

Learn more about photosynthesis here: brainly.com/question/3529377

#SPJ1

6 0
2 years ago
I need help asap!!!!
Butoxors [25]

Answer:

2H₂O₂ →  2H₂O + O₂

24.7 L are the liters of formed oxygen.

Explanation:

We state the reaction:

2H₂O₂ →  2H₂O + O₂

2 moles of peroxide decompose to 2 moles of water and 1 mol of oxygen gas.

We convert the mass to moles: 75 g . 1 mol / 34 g = 2.20 moles

As ratio is 2:1, per 2.20 moles of peroxide I would produce the half of moles, of O₂ → 2.20 /2 = 1.10 moles

We convert the moles to mass → 1.10 mol . 32 g / 1 mol = 35.3 g

Let's use oxygen's density to find out the volume

δ O₂ = 1.429 g/L    (mass/volume)

35.3 g . 1L / 1.429g = 24.7 L

6 0
3 years ago
Read 2 more answers
When a 1.00-g sample of methane gas was burned with excess oxygen in the calorimeter, the temperature increased by 7.3°C. When
Advocard [28]

Answer:

The energies of  combustion (per gram) for hydrogen and methane are as follows: Methane = 82.5 kJ/g;  Hydrogen = 162 kJ/g

<em>Note: The question is incomplete. The complete question is given below:</em>

To compare the energies of combustion of these fuels, the  following experiment was carried out using a bomb  calorimeter with a heat capacity of 11.3 kJ/℃.  When a 1.00-g sample of methane gas burned with

<em>excess oxygen in the calorimeter, the temperature  increased by 7.3℃. When a 1.00 g sample of  hydrogen gas was burned with excess oxygen, the temperature increase was 14.3°C. Compare the energies of  combustion (per gram) for hydrogen and methane.</em>

Explanation:

From the equation of the first law of thermodynamics, ΔU = Q + W

Since there is no expansion work in the bomb calorimeter,  ΔU = Q

But Q = CΔT

where C is heat capacity of the bomb calorimeter =  11.3
kJ/ºC; ΔT = temperature change

For combustion of methane gas:

Q per gram = (
11.3
kJ/ºC * 7.3°C)/1.0g

Q = 83 kJ/g

For combustion of hydrogen gas:

Q per gram = (
11.3
kJ/ºC * 14.3°C)/1.0g

Q = 162 kJ/g

3 0
3 years ago
What is a solvent?
NemiM [27]

Answer:

C. the substance in which the solute dissolves

Explanation:

There are two terms in this... the solute and the solvent. The way I learned how to remember this is with a little pirate analogy: The loot (stolen treasure) always goes in the vent. So, the soLUTE goes in the solVENT.

5 0
3 years ago
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