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3 years ago

Billy beaker traveled 115 kilometers in one morning: how far is this in feet

Chemistry

2 answers:

Pachacha [2.7K]3 years ago

8 0

Is the answer youre looking for 377297 feet

kotykmax [81]3 years ago

6 0

1 kilometer = 3280.84 feet.

So 115 kilometers = 3280.84 * 115 = 377296.6 feet

So Billy beaker traveled 377296.6 feet. If you wanted to round the answer, he traveled 377297 feet.

Hope this helps! :)

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Convert 25 degrees Celsius to Farenheit.

Sindrei [870]

Answer:

(25°C × 9/5) + 32 = 77°F

Explanation:

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2 years ago

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A 6.00 L vessel contains 20.0 g of PCl3 and 3.15 g of O2 at 15.0 ∘C. The vessel is heated to 210 ∘C, and the contents react to g

dusya [7]

Answer: The final pressure in the vessel will be 0.965 atm

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For phosphorus trichloride:

Given mass of phosphorus trichloride = 20.0 g

Molar mass of phosphorus trichloride = 137.3 g/mol

Putting values in equation 1, we get:

$\text{Moles of phosphorus trichloride}=\frac{20.0g}{137.3g/mol}=0.146mol$

For oxygen gas:

Given mass of oxygen gas = 3.15 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of oxygen gas}=\frac{3.15g}{32g/mol}=0.098mol$

The chemical equation for the reaction of phosphorus trichloride and oxygen gas follows:

$2PCl_3+O_2\rightarrow 2POCl_3$

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride reacts with 1 mole of oxygen gas

So, 0.146 moles of phosphorus trichloride will react with = $\frac{1}{2}\times 0.146=0.073mol$ of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, phosphorus trichloride is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride produces 2 moles of $POCl_3$

So, 0.146 moles of phosphorus trichloride will produce = $\frac{2}{2}\times 0.146=0.146mol$ of $POCl_3$

To calculate the pressure of the vessel, we use the equation given by ideal gas follows:

$PV=nRT$

where,

P = pressure of the vessel = ?

V = Volume of the vessel = 6.00 L

T = Temperature of the vessel = $210^oC=[210+273]K=483K$

R = Gas constant = $0.0821\text{ L. atm }mol^{-1}K^{-1}$

n = number of moles = 0.146 moles

Putting values in above equation, we get:

$P\times 6.00L=0.146mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 483K\\\\P=\frac{0.146\times 0.0821\times 483}{6.00}=0.965atm$

Hence, the final pressure in the vessel will be 0.965 atm

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ANEK [815]

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