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2 years ago

2CO(g) + O2(g) = 2CO2(g)

Chemistry

1 answer:

Finger [1]2 years ago

8 0

Answer:

3.0 L O₂

Explanation:

If CO reacts at STP, it means that there are 1.0 moles of CO. To find the moles of O₂, you need to use the mole-to-mole ratio from the given equation.

1.0 moles CO 1 mole O₂
---------------------- x --------------------- = 0.5 moles O₂
2 moles CO

To calculate the liters of oxygen, you need to use Avogadro's Law:

V₁ / N₁ = V₂ / N₂

In this equation, "V₁" and "N₁" represent the volume and moles of the first molecule. "V₂" and "N₂" represent the volume and moles of the second molecule. You can plug the given and calculated values into the equation and simplify to isolate V₂.

V₁ = 6.0 L V₂ = ? L

N₁ = 1.0 moles N₂ = 0.5 moles

V₁ / N₁ = V₂ / N₂ <----- Avogadro's Law

(6.0 L) / (1.0 moles) = V₂ / (0.5 moles) <----- Insert values

6.0 = V₂ / (0.5 moles) <----- Simplify left side

3.0 = V₂ <----- Multiply both sides by 0.5

**I am not 100% confident on this answer. Please let me know if it is incorrect**

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3 years ago

What is the salt produced when sulfuric acid (H2SO4) reacts with potassium hydroxide (KOH)?

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3 years ago

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He rate constant of a reaction is 4.55 × 10−5 l/mol·s at 195°c and 8.75 × 10−3 l/mol·s at 258°c. what is the activation energy o

Xelga [282]

Answer : The activation energy of the reaction is, $17.285\times 10^4kJ/mole$

Solution :

The relation between the rate constant the activation energy is,

$\log \frac{K_2}{K_1}=\frac{Ea}{2.303\times R}\times [\frac{1}{T_1}-\frac{1}{T_2}]$

where,

$K_1$ = initial rate constant = $4.55\times 10^{-5}L/mole\text{ s}$

$K_2$ = final rate constant = $8.75\times 10^{-3}L/mole\text{ s}$

$T_1$ = initial temperature = $195^oC=273+195=468K$

$T_2$ = final temperature = $258^oC=273+258=531K$

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Ea = activation energy

Now put all the given values in the above formula, we get the activation energy.

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3 years ago

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How many moles of CO2 must dissolve in excess water to produce 12 moles of<br><br> H2CO3?

vodka [1.7K]

Answer:

12 moles of CO₂.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

CO₂ + H₂O —> H₂CO₃

From the balanced equation above,

1 mole of CO₂ dissolves in water to produce 1 mole of H₂CO₃.

Finally, we shall determine the number of moles of CO₂ that will dissolve in water to produce 12 moles of H₂CO₃. This can be obtained as follow:

From the balanced equation above,

1 mole of CO₂ dissolves in water to produce 1 mole of H₂CO₃.

Therefore, 12 moles of CO₂ will also dissolve in water to produce 12 moles of H₂CO₃.

Thus, 12 moles of CO₂ is required.

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