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Fynjy0 [20]
1 year ago
11

Consider the reaction and its equilibrium constant at 25.0 ∘C :

Chemistry
1 answer:
olga55 [171]1 year ago
5 0

Since Qp>Kp , the reaction is not at equilibrium.

<h3>What is the equilibrium constant?</h3>

The equilibrium constant shows the extent to which reactants are converted into products.

Now we have to obtain the Qp as follows;

Qp =[CH3OH]/[CO] [H2]^2

Qp = 0.265/(0.265) (0.265)^2

Qp = 14.2

Now we know that Kp = 6.09×10−3, Since Qp>Kp , the reaction is not at equilibrium.

Learn more about equilibrium constant:brainly.com/question/10038290

#SPJ1

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Answer:

Hope this helps! (;_;)/

Explanation:

3 0
2 years ago
Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel ro
melamori03 [73]

<u>Answer:</u> The mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

  • <u>For nickel:</u>

Given mass of nickel = 14.8 g

Molar mass of nickel = 58.7 g/mol

Putting values in equation 1, we get:

\text{Moles of nickel}=\frac{14.8g}{58.7g/mol}=0.252mol

For the given chemical reaction:

3NiO(s)+2Al(s)\rightarrow 3Ni(l)+Al_2O_3(s)

  • <u>For nickel (II) oxide:</u>

By Stoichiometry of the reaction:

3 moles of nickel are produced from 3 moles of nickel (II) oxide

So, 0.252 moles of nickel will be produced from \frac{3}{3}\times 0.252=0.252mol of nickel (II) oxide

Now, calculating the mass of nickel (II) oxide by using equation 1:

Molar mass of nickel (II) oxide = 74.7 g/mol

Moles of nickel (II) oxide = 0.252 moles

Putting values in equation 1, we get:

0.252mol=\frac{\text{Mass of nickel (II) oxide}}{74.7g/mol}\\\\\text{Mass of nickel (II) oxide}=(0.252mol\times 74.7g/mol)=18.8g

  • <u>For aluminium:</u>

By Stoichiometry of the reaction:

3 moles of nickel are produced from 2 moles of aluminium

So, 0.252 moles of nickel will be produced from \frac{2}{3}\times 0.252=0.168mol of aluminium

Now, calculating the mass of aluminium by using equation 1:

Molar mass of aluminium = 27 g/mol

Moles of aluminium = 0.168 moles

Putting values in equation 1, we get:

0.168mol=\frac{\text{Mass of aluminium}}{27g/mol}\\\\\text{Mass of aluminium}=(0.168mol\times 27g/mol)=4.54g

Hence, the mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.

4 0
3 years ago
Hands moving on a battery-operated clock is an example of what kind of
Alexxandr [17]
The C is right answer
4 0
2 years ago
Read 2 more answers
How many bananas are equal to 7.50 moles of bananas?​
Veseljchak [2.6K]

Answer:

4.52×10^24

Explanation:

N = n × Na

where; N = no. of bananas

n = no. of moles

Na = Avogadro's constant

Which is 6.02×10^23

N = 7.5 × 6.02×10^23

N =4.515×10^24

7 0
2 years ago
16 meters per hour to miles per sec
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Answer:

2.76 (full answer) 2.7617e-6

Explanation:

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