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3 years ago

What is the density of oxygen gas (O2) at 2.3 atmospheres and 305 Kelvin? Show all of the work used to solve this problem.

Chemistry

1 answer:

sammy [17]3 years ago

5 0

Answer:

2.94g/L

Explanation:

First, let us derive an expression for the density, using the ideal gas equation:

PV = nRT (1)

V = nRT/ P (2)

Recall:

Number of mole(n) = mass(m)/Molar Mass (M)

n = m/M

Substituting the value of n into equation 2:

V = nRT/ P

V = mRT/ MP

Now Divide both side by m

V/m = RT/ MP

Inverting the above equation, we have:

m/V = MP/RT

But Density = m/V

Density = MP/RT

From the question given, we obtained the following data:

P = 2.3atm

T = 305K

Molar Mass of O2 = 16x2 = 32g/mol

R = 0.082atm.L/K /mol

Density = (32x2.3)/(0.082x305)

Density = 2.94g/L

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Wat is significant figures

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Answer:

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3 years ago

Give the answer to the problem below using the correct number of significant digits. (1.3 x 103) x (5.724 x 104)

Gemiola [76]

(133.9) x (595.296)= 79,710.1344
Answer with significant digits: 80,000
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6 0

3 years ago

Read 2 more answers

If Marie and Calvin dissolve 50 grams of KBr in 100 grams of water at 90oC, the solution is

hram777 [196]

Answer:

The solution is 50 %wt

Explanation:

50% wt is a sort of concentration and means, that 50 g of solute (in this case, the potassium bromide) dissolved in 100 g of water.

It is the same to say, that there are 50g of KBr for every 100g of H₂O

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3 years ago

Calculate the standard enthalpy change for the reaction at 25 ∘ C. Standard enthalpy of formation values can be found in this li

meriva

Answer:

The standard enthalpy change for the reaction at $25^{0}\textrm{C}$ is -2043.999kJ

Explanation:

Standard enthalpy change ( $\Delta H_{rxn}^{0}$ ) for the given reaction is expressed as:

$\Delta H_{rxn}^{0}=[3mol\times \Delta H_{f}^{0}(CO_{2})_{g}]+[4mol\times \Delta H_{f}^{0}(H_{2}O)_{g}]-[1mol\times \Delta H_{f}^{0}(C_{3}H_{8})_{g}]-[5mol\times \Delta H_{f}^{0}(O_{2})_{g}]$

Where $\Delta H_{f}^{0}$ refers standard enthalpy of formation

Plug in all the given values from literature in the above equation:

$\Delta H_{rxn}^{0}=[3mol\times (-393.509kJ/mol)]+[4mol\times (-241.818kJ/mol)]-[1mol\times (-103.8kJ/mol)]-[5mol\times (0kJ/mol)]=-2043.999kJ$

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2 years ago