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FromTheMoon [43]
2 years ago
7

2. What pressure is required to compress 196.0 L of air at 1.00 atmosphere into a cylinder

Chemistry
1 answer:
damaskus [11]2 years ago
3 0

Answer:

<h2>7.54 atm </h2>

Explanation:

The required pressure can be found by using the formula for Boyle's law which is

P_2 =  \frac{P_1V_1}{V_2}  \\

where

P1 is the initial pressure

P2 is the final pressure

V1 is the initial volume

V2 is the final volume

From the question we have

P_2 =  \frac{1 \times 196}{26}  =  \frac{196}{26}   \\ = 7.538461...

We have the final answer as

<h3>7.54 atm </h3>

Hope this helps you

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Can u write it more specifically? so that I can answer
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If 100.0g of nitrogen is reacted with 100.0g of hydrogen, what is the theoretical yield of the reaction? What is the excess reac
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theoretical yield of ammonia (NH₃) = 121.38 g

The limiting reactant is nitrogen (N₂) and the excess reactant is hydrogen (H₂).

Explanation:

We have the following chemical reaction in which nitrogen react with hydrogen to produce ammonia:

N₂ + 3 H₂ → 2 NH₃

Now we need to calculate the number of moles of each reactant:

number of moles = mass / molar weight

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number of moles of H₂ = 100 / 2 = 50 moles

We see from the chemical reaction that 3 moles of H₂ react with 1 mole of N₂ so 50 moles of H₂ react with 16.67 moles of N₂ which is way more than the available N₂ quantity of 3.57 moles, so the limiting reactant is nitrogen (N₂) and the excess reactant is hydrogen (H₂).

Knowing this we devise the following reasoning:

if                1 mole of N₂ produces 2 moles of NH₃

then   3.57 moles of N₂ produces X moles of NH₃

X = (3.57 × 2) / 1 = 7.14 moles of NH₃

mass =  number of moles × molar weight

mass of NH₃ = 7.14 × 17 = 121.38 g (theoretical yield)

Learn more about:

limiting reactant

brainly.com/question/14111505

#learnwithBrainly

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3 years ago
A solution of H2SO4(aq) with a molal concentration of 4.80 m has a density of 1.249 g/mL. What is the molar concentration of thi
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Imagine we have <span>mass of solvent 1kg (1000g)
According to that: </span>molality =n(solute) / m(solvent) =\ \textgreater \  4.8m = 4.8mole / 1kg
= 4.8 mole * 98 g/mole = 470g
m(H2SO4) = n(H2SO4)*Mr(H2SO4) =\ \textgreater \=\ \textgreater \  Molarity = 4.8 mole / 1.2 L = 4 M m(H2SO4)  which is =<span>470g

</span><span>m(solution) = m(H2SO4) + m(solvent) = 470 + 1000 = 1470 g
d(solution) = m(solution) / V(solution) =>
=> 1.249 g/mL = 1470 g / V(solution) =></span>
Molarity = n(solute) / V(solution) =\ \textgreater \
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