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zalisa [80]
3 years ago
10

When people conserve electricity, power plants do not need to produce as much electricity because there is less demand for it.

Chemistry
1 answer:
almond37 [142]3 years ago
5 0

True

Explanation:

When people conserve electricity, power plants do not need to produce as much electricity because there is less demand for it.

This very correct.

  • When electricity is used in a sustainable way, there is little of it consumed.
  • Switching off idle electronics would make that amount of electric current to be re-distributed to another place.
  • Less coal and fuel would be used and power plants do not need to produce as much electricity.
  • Most electricity produced in power plants are often wasted due to idle appliances consuming the bulk of them.
  • When these appliances are turned off, less energy is in demand and less will be produced.

learn more:

Conservation of resources brainly.com/question/8690489

#learnwithBrainly

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The chemical bonding in sodium phosphate, Na3PO4, is classified as:
fiasKO [112]
<span>Ionic bonding between sodium and phosphate ions.</span>
7 0
3 years ago
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Assume that the maximum number of ATPs is produced (38). At pH 7, and in the presence of excess Mg2 , how much of the energy in
Lubov Fominskaja [6]

In one mole of glucose 38 ATP energy is stored this accounts for only 40 per-cent of the total energy in glucose.

Explanation:

In standard conditions, during the cellular respiration 1 mole of Glucose in the presence of oxygen produces 36 or 38 ATPs. This accounts for only 40% of the total energy as the remaining 60 per-cent of the energy is dissipated as heat.

I mole of glucose enters the glycolysis step of aerobic cellular respiration which after oxidative phosphorylation and Electron transport chain would give 38 ATP molecules.

It can be said that only 38.3% of energy is put in ATP molecules.

8 0
3 years ago
The solubility of Cr(NO3)3⋅9H2O in water is 208 g per 100 g of water at 15 ∘C. A solution of Cr(NO3)3⋅9H2O in water at 35 ∘C is
Zinaida [17]

Answer:

102g of crystals

Explanation:

When the Cr(NO₃)₃⋅9H₂O is dissolved in water at 15°C, the maximum mass that water will dissolve in the equilibrium is 208 g per 100g of water. When you heat the water, this mass will increases.

In this problem, at 35°C the water dissolves 310g in 100g of water, as in the equilibrium at 15°C the maximum mass is 208g, the mass of crystals that will form is:

310g - 208g = <em>102g of crystals</em>

<em>-Crystals are the Cr(NO₃)₃⋅9H₂O that is not dissolved-.</em>

I hope it helps!

5 0
3 years ago
What is the molarity of a 2.4-liter solution containing 124 grams of HF?
ioda
Molar mass:

HF = 1 + 19 = 20.0 g/mol

Number of moles :

124 / 20.0 =>  6.2 moles

Volume = 2.4 L

M = n / V

M = 6.2 / 2.4

M = 2.6 M

Answer A

hope this helps!

7 0
3 years ago
Read 2 more answers
If 16.00 g of O₂ reacts with 80.00 g NO, how many the excess reactant are left over? (enter only the value, round to whole numbe
pishuonlain [190]

Answer:

50

Explanation:

We will need a balanced equation with masses, moles, and molar masses of the compounds involved.

1. Gather all the information in one place with molar masses above the formulas and masses below them.  

Mᵣ:           30.01     32.00   46.01

               2NO   +   O₂ ⟶ 2NO₂

Mass/g:  80.00     16.00

2. Calculate the moles of each reactant  

\text{moles of NO} = \text{80.00 g NO} \times \dfrac{\text{1 mol NO}}{\text{30.01 g NO}} = \text{2.666 mol NO}\\\\\text{moles of O}_{2} = \text{16.00 g O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{32.00 g O}_{2}} = \text{0.5000 mol O}_{2}

3. Calculate the moles of NO₂ we can obtain from each reactant

From NO:

The molar ratio is 2 mol NO₂:2 mol NO

\text{Moles of NO}_{2} = \text{2.333 mol NO} \times \dfrac{\text{2 mol NO}_{2}}{\text{2 mol NO}} = \text{2.333 mol NO}_{2}

From O₂:

The molar ratio is 2 mol NO₂:1 mol O₂

\text{Moles of NO}_{2} =  \text{0.5000 mol O}_{2}\times \dfrac{\text{2 mol NO}_{2}}{\text{1 mol Cl}_{2}} = \text{1.000 mol NO}_{2}

4. Identify the limiting and excess reactants

The limiting reactant is O₂ because it gives the smaller amount of NO₂.

The excess reactant is NO.

5. Mass of excess reactant

(a) Moles of NO reacted

The molar ratio is 2 mol NO:1 mol O₂

\text{Moles reacted} = \text{0.500 mol O}_{2} \times \dfrac{\text{2 mol NO}}{\text{1 mol O}_{2}} = \text{1.000 mol NO}

(b) Mass of NO reacted

\text{Mass reacted} = \text{1.000 mol NO} \times \dfrac{\text{30.01 g NO}}{\text{1 mol NO}} = \text{30.01 g NO}

(c) Mass of NO remaining

Mass remaining = original mass – mass reacted = (80.00 - 30.01) g = 50 g NO

5 0
3 years ago
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