What volume of oxygen gas at 25 degrees celsius and 1.04 atm is needed for the complete combustion of 5.53g of propane

Answers

Answer 1

Answer:

Answer: 14.7 L of oxygen gas at 25 degrees celsius and 1.04 atm is needed for the complete combustion of 5.53g of propane

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at NTP, weighs equal to the molecular mass and contains avogadro's number $6.023* 10^(23)$ of particles.

$\text{Number of moles of propane}=\frac{\text{Given mass}}{\text{Molar mass}}=(5.53g)/(44.1g/mol)=0.125moles$

$C_3H_8+5O_2\rightarrow 3CO_2+4H_2O$

According to stoichiometry :

1 mole of propane requires 5 moles of oxygen

Thus 0.125 moles of propane require= $(5)/(1)* 0.125=0.625moles$ moles of oxygen

According to the ideal gas equation:'

$PV=nRT$

P = Pressure of the gas = 1.04 atm

V= Volume of the gas = ?

T= Temperature of the gas = 25°C = 298 K

R= Gas constant = 0.0821 atmL/K mol

n= moles of gas= 0.625

$V=(nRT)/(P)=(0.625* 0.0821* 298)/(1.04)=14.7L$

Answer 2

Answer:

Final answer:

To find the volume of oxygen gas needed for the complete combustion of propane at given conditions, use stoichiometric calculations based on the balanced chemical equation and apply the ideal gas law.

Explanation:

The question is asking for the volume of oxygen gas required for the complete combustion of a given amount of propane at a specified temperature and pressure. To solve this, stoichiometry must be used along with the ideal gas law. The balanced chemical equation for the combustion of propane (C3H8) is:

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l)

This equation indicates that one mole of propane reacts with five moles of oxygen. First, calculate the moles of propane by dividing the given mass of propane by its molar mass. Then, use the stoichiometric relationship from the balanced equation to find the moles of oxygen needed. Finally, apply the ideal gas law (PV=nRT) to calculate the required volume of oxygen at the given conditions (remembering to convert temperature to Kelvin and pressure to atm if necessary).

Learn more about Stoichiometry here:

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Explanation:

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Answers

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What is the pOH of a 4.8x10^-10M H+ solution

Answers

Answer : The value of pOH of the solution is, 4.68

Explanation : Given,

Concentration of $H^+$ ion = $4.8* 10^(-10)M$

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If a gas occupies 22.4 L at 0.265 atm, then what will the pressure be in atmospheres if the gas occupies 35.52 L? Assume all othervariables are held constant
A)0.167 atm
B)0.437 atm
C)0.886 atm
D)149 atm

Answers

Answer:

The new pressure is 0.167 atm

The correct answer is option A

Explanation:

Step 1: Data given

Volume of the gas = 22.4 L

Pressure of the gas = 0.265 atm

The volume increases to 35.52 L

Step 2: Calculate the new pressure

P1*V1 = P2*V2

⇒with P1 = the initial pressure = 0.265 atm

⇒with V1 = the initial volume = 22.4 L

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with V2 = the increased volume = 35.52 L

0.265 atm * 22.4 L = P2 * 35.52 L

P2 = (0.265 atm * 22.4 L) / 35.52 L

P2 = 0.167 atm

The new pressure is 0.167 atm

The correct answer is option A

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