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DIA [1.3K]
2 years ago
12

Help me please (~ ̄_ ̄)~​

Chemistry
2 answers:
katen-ka-za [31]2 years ago
6 0

Answer:

<h3>The numerical value of equilibrium constant depends on</h3>

<h2><em>Temperature</em><em> </em></h2>

Explanation:

When the temperature increases, the value of the equilibrium constant decreases and when the temperature decreases then the equilibrium constant increases. So I think the answer should be Temperature

Lubov Fominskaja [6]2 years ago
5 0

Answer:

1.Temperature is the answer.

Explanation:

Hope this help!!

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How many moles of N2 are need to fill a 35 L tank at standard temperature and pressure?
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1.56 moles of N2 are needed to fill a 35 L tank at standard temperature and pressure. Details about moles can be found below.

<h3>How to calculate number of moles?</h3>

The number of moles of a substance can be calculated using the following formula:

PV = nRT

Where;

  • P = pressure
  • V = volume
  • n = number of moles
  • R = gas law constant
  • T = temperature

At STP;

  • T = 273K
  • P = 1 atm
  • R = 0.0821 Latm/molK

1 × 35 = n × 0.0821 × 273

35 = 22.41n

n = 35/22.41

n = 1.56mol

Therefore, 1.56 moles of N2 are needed to fill a 35 L tank at standard temperature and pressure.

Learn more about number of moles at: brainly.com/question/14919968

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2 years ago
Methylpentane is held in a closed container at 150°f. both gas and liquid are present. what is the pressure in the container
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Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide. Ca) + H2O --&gt; Ca(OH)2 In a particular
mars1129 [50]

Answer:

Percent yield = 92.5%

Explanation:

The question asks for the percent yield which can be defined as:

\frac{actual yield}{theoretical yield} .100

Where the actual yield is <em>how much product was obtained</em>, in this case 6.11 g of Ca(OH)₂, and the theoretical yield is <em>how much product could be obtained with the given reactants theoretically</em>, that is if the reaction would work perfectly. So we need to calculate first the theoretical yield.

1. First lets write the chemical equation reaction correctly and check that it is balanced:

CaO + H₂O → Ca(OH)₂

2. Calculate the amount of product Ca(OH)₂ that can be obtained with the given reactants (theoretical yield), which are 5.00g of CaO and excess of water. So the amount of CaO will determined how much Ca(OH)₂ we can obtained.

For this we'll use the molar ratio between CaO and Ca(OH)₂ which we see it is 1:1. For every mol of CaO we'll obtain a mol of Ca(OH)₂. So lets convert the 5.00 g of CaO to moles:

 Molar Mass of CaO: 40.078 + 15.999 = 56.077 g/mol

 moles of CaO = 5.00 g / 56.077 g/mol = 0.08916 moles

As we said before from the molar ratio moles of Ca(OH)₂ = moles of CaO

So the moles of Ca(OH)₂ that can be obtained are 56.077 g/mol

We need to convert this value to grams:

 Molar Mass of Ca(OH)₂ = 40.078 + (15.999 + 1.008)*2 = 74.092 g/mol

Theoretical yield of Ca(OH)₂ = 0.08916 moles x 74.092 g/mol = 6.606 g

3. Calculate the percent yield:

\frac{actual yield}{theoretical yield} .100

Percent yield = (6.11 g / 6.606g) x 100 = 92.5 %

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