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jenyasd209 [6]
2 years ago
13

What is the volume of 0.80 grams of o2 gas at stp? (5 points) group of answer choices 0.59 liters 0.56 liters 0.50 liters 0.47 l

iters
Chemistry
2 answers:
Vladimir [108]2 years ago
5 0

Answer:

0.56L

Explanation:

This question requires the Ideal Gas Law:  PV=nRT where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the Ideal Gas constant, and T is the Temperature of the gas.

Since all of the answer choices are given in units of Liters, it will be convenient to use a value for R that contains "Liters" in its units:R=0.0821\frac{L\cdot atm}{mol\cdot K}

Since the conditions are stated to be STP, we must remember that STP is Standard Temperature Pressure, which means T=273.15K and P=1atm

Lastly, we must calculate the number of moles of O_2(g) there are.  Given 0.80g of O_2(g), we will need to convert with the molar mass of O_2(g).  Noting that there are 2 oxygen atoms, we find the atomic mass of O from the periodic table (16g/mol) and multiply by 2:  32g\text{ }O_2=1mol\text{ }O_2

Thus, \frac{0.80g \text{ }O_2}{1} \frac{1mol\text{ }O_2}{32g\text{ }O_2}=0.25mol\text{ }O_2=n

Isolating V in the Ideal Gas Law:

PV=nRT

V=\frac{nRT}{P}

...substituting the known values, and simplifying...

V=\frac{(0.025 mol \text{ }O_2)(0.0821\frac{L\cdot atm}{mol \cdot K} )(273.15K)}{(1atm)}

V=0.56L \text{ } O_2

So, 0.80g of O_2(g) would occupy 0.56L at STP.

Jlenok [28]2 years ago
3 0

Answer:

0.56 L

Explanation:

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A balloon occupies 1.50 L with 0.205 mol of carbon dioxide. How many moles would be required to increase the size of the balloon
Gekata [30.6K]

Answer:

0.683 moles of the gas are required

Explanation:

Avogadro's law relates the moles of a gas with its volume. The volume of a gas is directely proportional to its moles when temperature and pressure of the gas remains constant. The law is:

V₁n₂ = V₂n₁

<em>Where V is volume and n are moles of 1, initial state and 2, final state of the gas.</em>

<em />

Computing the values of the problem:

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8 0
3 years ago
What is the ratio of lactic acid (Ka = 1.37x10-4) to lactate in a solution with pH =4.49?
Natasha2012 [34]
When Ka =1.37 x 10^-4 

∴Pka = - ㏒Ka

          = -㏒ 1.37 x 10^-4 
          
           = 3.86

According to H- H equation: 

when PH = PKA + ㏒[conjugate base / weak acid]

when the lactate is the conjugate base and lactic acid is the weak acid 

∴ PH = Pka +㏒[lactate] / [lactic acid]

so, by substitution:


4.49 = 3.86 + ㏒[lactate]/[lactic acid]

∴[lactate]/[lactic acid] = 4.3

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3 years ago
___CH4 + ___O2 → ___CO2 + ___H2O When you burn natural gas in the laboratory, methane burns. What numbers fill in the blanks to
Hitman42 [59]

Answer:

The coefficient are 1,2,1,2 ( option B is correct)

Explanation:

Step 1: Data given

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Burning methane = CH4 + O2

Step 2: The unbalanced equation

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Step 3: Balancing the equation

CH4(g) + O2(g) → CO2(g) + H2O(g)

On the left side we have 4x H (in CH4), on the right side we have 2x H (in H2O). To balance the amount of H, on both sides, we have to multiply H2O (on the right side by 2).

CH4(g) + O2(g) → CO2(g) + 2H2O(g)

On the left side we have 2x O (in O2), on the right side we have 4x O (2x in CO2 and 2x in 2H2O). To balance the amount of O on both sides, we have to multiply O2 (on the left side by 2).

CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

The coefficient are 1,2,1,2 ( option B is correct)

3 0
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