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Brilliant_brown [7]
2 years ago
15

A gaseous product of a reaction is collected at 280K and 0.95 atm. Given R=0.0821L⋅atmmol⋅K, what is the molar mass of the gas,

in grams per mole, if 5.49 g of gas occupies 4.92 L?
A. 0.04 g/mol

B. 133 g/mol

C. 24 g/mol

D. 27 g/mol
Chemistry
2 answers:
exis [7]2 years ago
8 0

Answer:

I took the test, see below

Explanation:

1. The volume increases to twice its original value.

2. volume & temperature are directly proportional

volume & pressure are inversely proportional

pressure & temperature are directly proportional

3. Gay-Lussac’s law, by seeing how changes in temperature affect the pressure of the gas

4.V1P1/T1=V2P2/T2

5. It is a straight line with a positive slope showing that an increase in temperature results in an increase in volume.

6. keeping the pressure constant and increasing the temperature

7. When temperature is held constant and volume increases, the pressure increases.

8. pressure, volume, temperature, number of moles

9. volume

10. 7.10 L/mol

11. 0.105 mol

12. 27 g/mol

13. the temperature increasing by a factor of 2

The rest are short answers, just give those your best shot.

White raven [17]2 years ago
6 0

The molar mass of the gas in grams per mole is 27 g/mol

The correct answer to the question is Option D. 27 g/mol

To solve this question, we'll begin by calculating the number of mole of the gas. This can be obtained as follow:

Temperature (T) = 280 K

Pressure (P) = 0.95 atm

Volume (V) = 4.92 L

Gas constant (R) = 0.0821 L⋅atm/mol⋅K

<h3>Number of mole (n) =? </h3>

<h3>PV = nRT </h3>

0.95 × 4.92 = n × 0.0821 × 280

4.674 = n × 22.988

Divide both side by 22.988

n = 4.674 / 22.988

<h3>n = 0.203 mole </h3>

Thus, the number of mole of the gas is 0.203 mole.

Finally, we shall determine the molar mass of the gas. This can be obtained as follow:

Number of mole of gas = 0.203 mole.

Mass of gas = 5.49 g

<h3>Molar mass =? </h3>

Mole = mass / molar mass

0.203 = 5.49 / molar mass

Cross multiply

0.203 × molar mass = 5.49

Divide both side by 0.203

Molar mass = 5.49 / 0.203

<h3>Molar mass = 27 g/mol </h3>

Therefore, the molar mass of the gas is 27 g/mol

Option D. 27 g/mol gives the correct answer to the question.

Learn more:

brainly.com/question/10542057

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Im hvaing a hard time getting the right answer
Tanya [424]

Answer:

V=23.9mL

Explanation:

Hello!

In this case for the solution you are given, we first use the mass to compute the moles of CuNO3:

n=2.49g*\frac{1mol}{125.55 g}=0.0198mol

Next, knowing that the molarity has units of moles over liters, we can solve for volume as follows:

M=\frac{n}{V}\\\\V=\frac{n}{M}

By plugging in the moles and molarity, we obtain:

V=\frac{0.0198mol}{0.830mol/L}=0.0239L

Which in mL is:

V=0.0239L*\frac{1000mL}{1L}\\\\V=23.9mL

Best regards!

6 0
3 years ago
An acid with molar mass 84.48 g/mol is titrated with 0.650 M KOH. What volume of KOH solution is needed to titrate 1.70 grams of
RSB [31]

Answer:

V=0.0310L=3.10mL

Explanation:

Hello.

In this case, since the acid is monoprotic and the KOH has one hydroxyl ion only, we can see that at the equivalence point the moles of both of them are the same:

n_{acid}=n_{KOH}

Thus, since we are given 1.70 g of the acid, we compute the moles of acid that were titrated:

n_{acid}=1.70g*\frac{1mol}{84.48g}=0.0201mol

Which equal the moles of KOH. In such a way, since the molarity is defined as moles over liters (M=n/V), the liters are moles over molarity (V=n/M), thus, the resulting volume is:

V=\frac{0.0201mol}{0.650mol/L}\\\\V=0.0310L=3.10mL

Best regards!

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Answer:

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