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3 years ago

How is a nonrenewable source different from a renewable one

1 answer:

5 0

A Nonrewnewable source is hard to get back from its source, while a renewable source is easy to get back from its source.

Example:

Nonrenewable: crude oil, oil, coal, fossil fuels, etc.

Renewable: sunlight, wind, biomass, rain, tides, waves and geothermal heat, etc.

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Equal amounts of N2 and O2 are added, under certain conditions, to a closed container. Which changes occur in the reverse reacti

geniusboy [140]

1) The forward reaction is N2 (g) + O2 (g) → 2NO

(that reaction requires special contitions because at normal pressures and temperatures N2 and O2 do not react to form another compound.

2) The equiblibrium equation is

N2 (g) + O2 (g) ⇄ 2NO

3) Then, the reverse reaction is

2NO → N2(g) + O2(g)

Answer: 2NO → N2(g) + O2(g)

4 0

3 years ago

Write the balanced chemical equations for the reaction of magnesium metal with oxygen gas, and for the reaction of magnesium met

Sunny_sXe [5.5K]

Magnesium element exists as single atoms. Free oxygen is always diatomic (two atoms bonded together) as O2. Nitrogen gas is also diatomic N2.

2Mg + O2 → MgO

Mg forms a +2 ion, O forms a -2 ion, so they combine and balance in a 1:1 ratio. MgO, magnesium oxide, is a solid.
3Mg + N2→Mg3N2

Mg forms a +2 ion, but N forms a -3 ion. Hence the Mg3N2 configuration for magnesium nitride.

4 0

3 years ago

Some important points for hadpicking<br>

Svet_ta [14]

Answer:

Handpicking right?

It is a very simple and easy method of separation. It doesn't require any kind of equipment to proceed. It takes very less time when performed for small quantity of mixture. It doesn't require any kind of preparation

8 0

2 years ago

BrainlieSTTTTTT A gas is originally stored at a pressure of 25 atm with a volume of 3 L. If the pressure were increased to 75 at

Crazy boy [7]

Explanation:

Apply Boyle's Law :-

P1V1 = P2V2

Where P1 is 25 atm
V1 is 3L
P2 is 75 atm
V2 is what we need to find out.

25 × 3 = 75 × V2

$\tt{V_2 = \dfrac{ 25 \times 3}{75}}$

$\tt{V_2 = \dfrac{75}{75}}$

<u>So, the answer is d) Part, 1L .</u>

Hope it helps :)

3 0

3 years ago

Hydrogen gas can be formed by the reaction of methane with water according to the equation.

Jet001 [13]

Answer:

60.9 % is the yield of the reaction

Explanation:

The reaction is: CH₄ + H₂O → CO + 3H₂

Let's apply the Ideal Gas Law to determine the moles of each reactant.

First of all, we convert the pressure from Torr to atm

732 Torr . 1atm / 760Torr = 0.963 atm Pressure of CH₄

702 Torr . 1atm / 760Torr = 0.923 atm Pressure of H₂O vapor

Now we can apply P . V = n . R . T

We convert T° from °C to K → 25°C + 273 = 298 K and 125°C + 273 = 398K

CH₄ → (25.5L . 0.963 atm) / 0.082 . 298K = n → 1 mol

H₂O vapor → (22.8L . 0.923 atm) / 0.082 . 398K = n → 0.64 mol

Ratio is 1:1, so the limiting reactant is the water vapor. I need 1 mol to react with 1 mol of methane but I only have 0.64 moles.

At the 100 % yield, 0.64 moles of water vapor may produce (0.64 . 3) = 1.92 moles of H₂.

We apply the P . V = n .R . T to determine the moles of H₂ produced at STP

1 atm . 26.2L = n . 0.082 . 273K

(1 atm . 26.2L) / (0.082 . 273K) = n → 1.17 moles of H₂

Percent yield of the reaction is (Yield produced / Theoretical yield) . 100

(1.17 moles / 1.92 moles) . 100 = 60.9%

3 0

2 years ago