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ahrayia [7]
3 years ago
12

Balance this equation Fe2O2 + C -> Fe + CO2​

Chemistry
2 answers:
lidiya [134]3 years ago
8 0

2 FeO + 1 C ===》2 Fe + 1 CO2

Akimi4 [234]3 years ago
3 0

Explanation:

Fe2O2+C-----> 2Fe+CO2

balanced equation..

hope it helps.

<h2>stay safe healthy and happy<u>.</u><u>.</u><u>.</u><u>.</u><u>.</u><u>.</u><u>.</u></h2>
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5. The density of ethanol is 0.789 g/mL. Find the mass of a sample of ethanol that has a volume of 150.0 mL.
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Compare S (secondary) waves and P (primary) waves. Why do they travel at different speeds?
Amanda [17]

S waves

  • These are shear waves .
  • The motion of the medium is perpendicular to  direction of propagation of the wave .
  • They can propagate only through solids and not through gases or liquids .
  • S waves are larger .
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P waves

  • These are compression waves .
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  • P waves are smaller than s waves .
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P-waves travel 60% faster than S-waves on average because the interior part of the Earth does not react the same way as the s wave and P wave.

8 0
3 years ago
How much NaOH (in grams) is needed to prepare 463 mL of solution with a pH of 10.020?
tino4ka555 [31]

Answer: 1.94\times 10^{-3}g of NaOH

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

pH=-\log [H^+]

Putting in the values:

10.020=-\log[H^+]

[H^+]=9.55\times 10^{-11}

[H^+][OH^-]=10^{-14}

[OH^-]=\frac{10^{-14}}{9.55\times 10^{-11}}=1.05\times 10^{-4}M

NaOH\rightarrow Na^++OH^-

Molarity=\frac{moles\times 1000}{\text {Volume in ml}}

1.05\times 10^{-4}M=\frac{moles\times 1000}{463ml}

moles = 4.86\times 10^{-5}

Mass of NaOH=moles\times {\text {Molar mass}}=4.86\times 10^{-5}\times 40=1.94\times 10^{-3}g

Thus 1.94\times 10^{-3}g of NaOH is needed to prepare 463 mL of solution with a pH of 10.020

8 0
3 years ago
I just need help on c-g. The whole question is there in case anyone needs it.
Elza [17]

Answer:

(c) 0.11; (d) -24.5 kJ·mol⁻¹; (e) See below; (f) Kc increases;

(g) No effect on ΔH

Step-by-step explanation:

(c) Kc at 125 °C  

In Part (a) one molecule of XY dissociated into one X and one Y.

       XY ⇌ X + Y

I:      10       0    0

C:     -1       +1   +1

E:      9        1     1

Kc = {[X][Y]}/[XY] = (1 × 1)/9 = ⅑ = 0.11

(d) ΔH

ΔH is a constant that is characteristic of the reaction.

ΔH = -24.5 kJ·mol⁻¹

(e) Effect of temperature on concentrations

If ΔH is negative, the reaction is exothermic.

Heat is a product of the reaction, so we can write the equation as

XY ⇌ X + Y + heat

If we lower the temperature, we are removing heat from the system.

<em>Le Châtelier's Principle</em> states that if you apply a stress to a system at equilibrium, it will respond by trying to relieve the stress.

We applied a stress by removing heat, so the system responds by producing more heat. The position of equilibrium moves to the right, and <em>more products will form</em>.

The diagram might look like the one below.

(f) Effect of temperature on Kc

Kc = [Products]/[Reactants]

We are increasing [Products] and decreasing [Reactants].

If you increase the numerator and decrease the denominator, you i<em>ncrease</em> the value of the quotient.

The value of the equilibrium constant increases when the temperature decreases.

(g) Effect of temperature on ΔH

Decreasing the temperature has no effect on ΔH, because the enthalpies of the reactants and products are properties of the substances themselves. They do not depend on the temperature.

7 0
3 years ago
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