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2 years ago

7.744 Liters of nitrogen are contained in a container. Convert this amount to grams.

Chemistry

1 answer:

Xelga [282]2 years ago

7 0

Answer:

9.69g

Explanation:

To obtain the desired result, first let us calculate the number of mole of N2 in 7.744L of the gas.

1mole of a gas occupies 22.4L at stp.

Therefore, Xmol of nitrogen gas(N2) will occupy 7.744L i.e

Xmol of N2 = 7.744/22.4 = 0.346 mole

Now let us convert 0.346 mole of N2 to gram in order to obtain the desired result. This is illustrated below:

Molar Mass of N2 = 2x14 = 28g/mol

Number of mole N2 = 0.346 mole

Mass of N2 =?

Mass = number of mole x molar Mass

Mass of N2 = 0.346 x 28

Mass of N2 = 9.69g

Therefore, 7.744L of N2 contains 9.69g of N2

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How many molecules of carbon dioxide are in 243.6 g of carbon dioxide?

german

Hey there !

Molar mass carbon dioxide:

CO2 = 44.01 g/mol

1) number of moles :

1 mole CO2 ------------- 44.01 g
(moles CO2) ------------ 243.6 g

moles CO2 = 243.6 * 1 / 44.01

moles CO2 = 243.6 / 44.01

=> 5.535 moles of CO2

Therefore:

1 mole -------------------- 6.02x10²³ molecules
5.535 moles ------------ ( molecules CO2)

molecules CO2 = 5.535 * ( 6.02x10²³) / 1

=> 3.33x10²⁴ molecules of CO2

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2 years ago

The density of liquid Z is 0.9237 g/mL. A student masses a cup

Ulleksa [173]

Answer:

37.65mL

Explanation:

Given parameters:

density of liquid Z = 0.9237g/mL

Mass of liquidZ + mass of cup = 50.7g

Mass of cup= 15.92g

Volume of liquid Z in cup=?

Solution:

Density is the mass per unit volume of a substance. It is mathematically expressed as shown below:

Density = $\frac{mass}{volume}$

To find the volume of liquid Z, we know the density of the liquid but we dont know the mass yet.

Mass of liquidZ = 50.7g - mass of cup = 50.7g - 15.92g = 34.98g

Therefore:

Volume of liquidZ = $\frac{mass of liquidZ}{density of liquidZ}$

= $\frac{34.98}{0.9237}$

= 37.65mL

3 0

2 years ago

Part a how many grams of xef6 are required to react with 0.579 l of hydrogen gas at 6.46 atm and 45°c in the reaction shown belo

Nina [5.8K]

First, let us find the corresponding amount of moles H₂ assuming ideal gas behavior.

PV = nRT
Solving for n,
n = PV/RT
n = (6.46 atm)(0.579 L)/(0.0821 L-atm/mol-K)(45 + 273 K)
n = 0.143 mol H₂

The stoichiometric calculations is as follows (MW for XeF₆ = 245.28 g/mol)
Mass XeF₆ = (0.143 mol H₂)(1 mol XeF₆/3 mol H₂)(245.28 g/mol) = <em>11.69 g</em>

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Answer:

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