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2 years ago

Write a balanced chemical equation depicting the formation of one mole of H2O2(g) from its elements in their standard states.

Chemistry

1 answer:

I am Lyosha [343]2 years ago

7 0

Answer:

$H_2(g)+O_2(g)\rightarrow H_2O_2(g)$

Explanation:

Hello!

In this case, since the formation reaction of a compound is undergone when the pure elements composing it are combined, for gaseous hydrogen peroxide, gaseous diatomic hydrogen and oxygen (standard state) must be combined in order to obtain the gaseous hydrogen peroxide as shown below:

$H_2(g)+O_2(g)\rightarrow H_2O_2(g)$

Whereas it is proved there are two hydrogen and oxygen atoms at each side of the chemical equation and therefore it is balanced.

Best regards!

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What volume of a 0.716 m kbr solution is needed to provide 30.5 g of kbr?

Jlenok [28]

Answer is: volume of KBr is 357 mL.
c(KBr) = 0,716 M = 0,716 mol/L.
m(KBr) = 30,5 g.
n(KBr) = m(KBr) ÷ M(KBr).
n(KBr) = 30,5 g ÷ 119 g/mol.
n(KBr) = 0,256 mol.
V(KBr) = n(KBr) ÷ c(KBr).
V(KBr) = 0,256 mol ÷ 0,716 mol/L.
V(KBr) = 0,357 L · 1000 mL/L = 357 mL.

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Answer:

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2 years ago

Calculate the enthalpy of combustion, δh∘comb, for c6h14. you'll first need to determine the balanced chemical equation for the

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2 years ago

12. The vapor pressure of water at 90°C is 0.692 atm. What is the vapor pressure (in atm) of a solution made by dissolving 3.68

luda_lava [24]

Answer : The vapor pressure (in atm) of a solution is, 0.679 atm

Explanation : Given,

Mass of $H_2O$ = 1.00 kg = 1000 g

Moles of $CsF$ = 3.68 mole

Molar mass of $H_2O$ = 18 g/mole

Vapor pressure of water = 0.692 atm

First we have to calculate the moles of $H_2O$ .

$\text{Moles of }H_2O=\frac{\text{Mass of }H_2O}{\text{Molar mass of }H_2O}=\frac{1000g}{18g/mole}=55.55mole$

Now we have to calculate the mole fraction of $H_2O$

$\text{Mole fraction of }H_2O=\frac{\text{Moles of }H_2O}{\text{Moles of }H_2O+\text{Moles of }CsF}=\frac{55.55}{55.55+3.68}=0.938$

Now we have to partial pressure of solution.

According to the Raoult's law,

$P_{Solution}=X_{H_2O}\times P^o_{H_2O}$

where,

$P_{Solution}$ = vapor pressure of solution

$P^o_{H_2O}$ = vapor pressure of water = 0.692 atm

$X_{H_2O}$ = mole fraction of water = 0.938

$P_{Solution}=X_{H_2O}\times P^o_{H_2O}$

$P_{Solution}=0.938\times 0.692atm$

$P_{Solution}=0.649atm$

Therefore, the vapor pressure (in atm) of a solution is, 0.679 atm

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2 years ago

If two unidentified solids of the same texture and color have different solubilities in 100 grams of water at 20°C, you could co

AlekseyPX

I'm certain it's "D"

...because it can't be "A" or "B" because solubility IS a property but to actually determine whether these two substances are the same or different we would need at least two-three properties (like boiling point or specific heat).

and it can't be "C" because the melting point is just simply irrelevant when comparing the solubility of two substances.

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