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choli [55]
3 years ago
15

3.75 g of an unknown gas at 59 °C and 1.00 atm is stored in a 1.35-L flask. What is the molar mass of the gas?

Chemistry
1 answer:
MAXImum [283]3 years ago
4 0
You need to find moles of the gas, so you would use the ideal gas law:
PV=nRT
Pressure
Volume
n=moles
R= gas constant
Tenperature in Kelvin
n= PV/RT
(1.00atm)(1.35L)/(.08206)(332K) = 0.050mol
Molar mass is grams per mole, so
(3.75g/.050mol) = 75g/mol
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A 7.5 L cylinder contains 5 moles of gas at a temperature of 274°C. What is its pressure in kiloPascals (kPa)?
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<h3><u>Answer;</u></h3>

 = 3032.15 kPa

<h3><u>Explanation;</u></h3>

Using the equation;

PV = nRT , where P is the pressure,. V is the volume, n is the number of moles and T is the temperature and R is the gas constant, 0.08206 L. atm. mol−1.

Volume = 7.5 L, T = 274 +273 = 547 K, N = 5 moles

Therefore;

Pressure = nRT/V

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But; 1 atm = 101325 pascals

Hence; Pressure = 3032150.63 pascals

                            <u>= 3032.15 kPa</u>

               

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How many moles of iron(III) hydroxide precipitate will form when 2.7 moles of aqueous sodium hydroxide reacts completely with ex
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Answer:

0.9 mole of Fe(OH)3.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

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Now, we can determine the moles of iron (III) hydroxide formed from the reaction as follow:

From the balanced equation above,

3 moles of NaOH reacted to produce 1 mole of Fe(OH)3.

Therefore, 2.7 moles of NaOH will react to produce = 2.7/3 = 0.9 mole of Fe(OH)3.

Therefore, 0.9 mole of Fe(OH)3 is produced from the reaction.

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3 years ago
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