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2 years ago

14

Does biomass energy come from petroleum?

1 answer:

IrinaK [193]2 years ago

7 0

No,Biomass is organic material which has stored sunlight in the form of chemical energy. Biomass fuels include wood, wood waste, straw, manure, sugar cane, and many other byproducts from a variety of agricultural processes. Biomass is a renewable energy source because the energy it contains comes from the sun<span>.</span>

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If a sample of NH3 gas at 689,1 mmHg has a volume of 607 2 mL and the presure is

never [62]

Answer:

The answer to your question is V2 = 746.1 ml

Explanation:

Data

Pressure 1 = P1 = 689.1 mmHg

Volume 1 = V1 = 607.2 ml

Pressure 2 = P2 = 560.8 mmHg

Volume 2 = V2 = ?

Process

To solve this problem use Boyle's law

P1V1 = P2V2

-Solve for V2

V2 = P1V1/P2

-Substitution

V2 = (689.1 x 607.2) / 560.8

-Simplification

V2 = 746.1 ml

8 0

2 years ago

Given the reaction: N2 + O2 = 2NO for which the Keq at 2273 K is 1.2 x 10-4

MAXImum [283]

<u>Answer:</u>

(a): The expression of equilibrium constant is $K_{eq}=\frac{[NO]^2}{[N_2][O_2]}$

(b): The equation to solve the concentration of NO is $[NO]=\sqrt{K_{eq}\times [N_2]\times [O_2]}$

(c): The concentration of NO is 0.0017 M.

<u>Explanation:</u>

The equilibrium constant is defined as the ratio of the concentration of products to the concentration of reactants raised to the power of the stoichiometric coefficient of each. It is represented by the term $K_{eq}$

(a):

The given chemical equation follows:

$N_2+O_2\rightarrow 2NO$

The expression for equilbrium constant will be:

$K_{eq}=\frac{[NO]^2}{[N_2][O_2]}$

(b):

The equation to solve the concentration of NO follows:

$[NO]=\sqrt{K_{eq}\times [N_2]\times [O_2]}$ ......(1)

(c):

Given values:

$K_{eq}=1.2\times 10^{-4}$

$[N_2]_{eq}=0.166M$

$[O_2]_{eq}=0.145M$

Plugging values in equation 1, we get:

$[NO]=\sqrt{(1.2\times 10^{-4})\times 0.166\times 0.145}$

$[NO]=\sqrt{2.88\times 10^{-6}}$

$[NO]=0.0017 M$

Hence, the concentration of NO is 0.0017 M.

3 0

2 years ago

2L of hydrogen has an initial pressure of 750 mmHg, what is the final pressure in mmHg if the volume increases to 20 L with a co

Verdich [7]

Answer: The final pressure is 75 mm Hg.

Explanation:

According to Boyle's law, at constant temperature the pressure of a gas in inversely proportional to volume.

Since, it is given that the temperature is constant. Hence, formula used is as follows.

$P_{1}V_{1} = P_{2}V_{2}$

Substitute the values into above formula as follows.

$P_{1}V_{1} = P_{2}V_{2}\\750 mm Hg \times 2 L = P_{2} \times 20 L\\P_{2} = \frac{750 mm Hg \times 2 L}{20 L}\\= 75 mm Hg$

Thus, we can conclude that the final pressure is 75 mm Hg.

3 0

2 years ago

Why do they call Cleveland "the mistake by the lake"?

algol13

Mostly because the lake smell really bad and the waters really dirty

3 0

2 years ago

Diatomic iodine [I2] decomposes at high temperature to form I atoms according to the reaction I2(g)⇌2I(g), Kc = 0.011 at 1200∘C

umka2103 [35]

Answer:

The concentration of I at equilibrium = 3.3166×10⁻² M

Explanation:

For the equilibrium reaction,

I₂ (g) ⇄ 2I (g)

The expression for Kc for the reaction is:

$K_c=\frac {\left[I_{Equilibrium} \right]^2}{\left[I_2_{Equilibrium} \right]}$

Given:

$\left[I_2_{Equilibrium} \right]$ = 0.10 M

Kc = 0.011

Applying in the above formula to find the equilibrium concentration of I as:

$0.011=\frac {\left[I_{Equilibrium} \right]^2}{0.10}$

So,

$\left[I_{Equilibrium} \right]^2=0.011\times 0.10$

$\left[I_{Equilibrium} \right]^2=0.0011$

$\left[I_{Equilibrium} \right]=3.3166\times 10^{-2}\ M$

<u>Thus, The concentration of I at equilibrium = 3.3166×10⁻² M</u>

3 0

2 years ago