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3 years ago

14

At what pressure, in atm, will 1.8 mol O₂ occupy a volume of 56.0 L at 35°C? Round your answer to the nearest hundredths. Don't

forget to label your units.

1 answer:

lubasha [3.4K]3 years ago

5 0

Answer:

Why has no one answered? Its been 4 days, I would if I knew it

Explanation:

Im taking the points so I stop seeing this~

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Sulfur dioxide, SO 2 ( g ) , can react with oxygen to produce sulfur trioxide, SO 3 ( g ) , by the reaction 2 SO 2 ( g ) + O 2 (

aleksley [76]

<u>Answer:</u> The amount of heat produced by the reaction is -21.36 kJ

<u>Explanation:</u>

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles.

The equation used to calculate enthalpy change is of a reaction is:

$\Delta H^o_{rxn}=\sum [n\times \Delta H_f_{(product)}]-\sum [n\times \Delta H_f_{(reactant)}]$

For the given chemical reaction:

$2SO_2(g)+O_2(g)\rightarrow 2SO_3(g)$

The equation for the enthalpy change of the above reaction is:

$\Delta H_{rxn}=[(2\times \Delta H_f_{(SO_3(g))})]-[(2\times \Delta H_f_{(SO_2(g))})+(1\times \Delta H_f_{(O_2(g))})]$

We are given:

$\Delta H_f_{(SO_2(g))}=-296.8kJ/mol\\\Delta H_f_{(SO_3(g))}=-395.7kJ/mol\\\Delta H_f_{(O_2(g))}=0kJ/mol$

Putting values in above equation, we get:

$\Delta H_{rxn}=[(2\times (-395.7))]-[(2\times (-296.8))+(1\times (0))]\\\\\Delta H_{rxn}=-197.8kJ/mol$

To calculate the number of moles, we use ideal gas equation, which is:

$PV=nRT$

where,

P = pressure of the gas = 1.00 bar

V = Volume of the gas = 2.67 L

n = number of moles of gas = ?

R = Gas constant = $0.0831\text{ L. bar }mol^{-1}K^{-1}$

T = temperature of the mixture = $25^oC=[25+273]K=298K$

Putting values in above equation, we get:

$1.00bar\times 2.67L=n\times 0.0831\text{ L. bar }mol^{-1}K^{-1}\times 298K\\\\n=\frac{1\times 2.67}{0.0831\times 298}=0.108mol$

To calculate the heat released of the reaction, we use the equation:

$\Delta H_{rxn}=\frac{q}{n}$

where,

q = amount of heat released = ?

n = number of moles = 0.108 moles

$\Delta H_{rxn}$ = enthalpy change of the reaction = -197.8 kJ/mol

Putting values in above equation, we get:

$-197.8kJ/mol=\frac{q}{0.108mol}\\\\q=(-197.8kJ/mol\times 0.108mol)=-21.36kJ$

Hence, the amount of heat produced by the reaction is -21.36 kJ

3 0

3 years ago

Wht is the boiling point of plastic

Schach [20]

Of the six commonly recycled plastics, four can withstand temperatures of 100 degrees Celsius (212 degrees Fahrenheit) or above. According to Machinist Materials, polyethylene terephthalate -- PET, or recyclable 1 -- has a melting point of 255 degrees Celsius (491 degrees Fahrenheit).

6 0

3 years ago

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The diagram shows salt dissolved in water. What does it show about water molecules

Rufina [12.5K]

Answer:

that they all dissolved went on watef

7 0

3 years ago

The process in which an organic acid and an alcohol react to form an ester and water is known as esterification. Ethyl butanoate

Daniel [21]

Answer:

696g

Explanation:

To determine the mass of ethylbutanoate produced, it is important that we know the number of moles of ethylbutanoate produced.

Now from the chemical equation, it can be seen that one mole of ethanol produces one mole of ethylbutanoate. This means that 6.0 mol of ethanol will surely produce 6.0 mol of ethylbutanoate.

Now, we need to get the mass of ethylbutanoate produced. The mass of ethylbutanoate produced is the number of moles of ethylbutanoate produced multiplied by the molar mass of ethylbutanoate produced.

The molar mass of ethylbutanoate is 12(6) + 12(1) + 16(2) = 116g/mol

The mass thus produced is 116 * 6 = 696g

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4 years ago

6. Which of the following units would be MOST appropriate for measuring

Sindrei [870]

Answer:

Meter

Explanation:

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3 years ago