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3 years ago

A sample of neon occupies a volume of 375 ml at stp. What will be the volume of neon If the pressure is reduced to 90.0 KPA?

Chemistry

2 answers:

Leokris [45]3 years ago

5 0

At STP conditions value of absolute pressure is 101.325 kPa.

From the given data we can determine the new volume of neon using following proportion:

V : V1 = p : p1

375 : V1 = 101.325 : 90

101 * V1 = 90 * 375

V1 =33750/101 =333ml

abruzzese [7]3 years ago

4 0

Since neon is a noble gas we can easily assume its behaviour to be an ideal gas. In ideal gases pressure is said to be inversely proportional to volume,
at fixed temperature, this is Boyle's law.

Therefore we can use this law to state the following equation
P1V1/T1 = P2V2/T2
in this case temperature is fixed therefore it can be eliminated,
then,
P1V1 = P2V2
standard pressure (P1) is 101 325 Pa
V1 = 375 ml
P2 = 90 000 Pa
substituting these values,
101 325 Pa * 375 ml = 90 000 Pa * V2
V2 = 101 325 * 375 / 90 000
= 422.18 ml
After rounding off the final answer is option A - 422 ml

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3 years ago

Two isotopes of lithium are found in nature Li6 has a mass of 6. 02u and Li7 has a mass of 7.02u . Use the atomic weight of lith

alexandr402 [8]

The isotope that is more abundant, given the data is isotope Li7

<h3>Assumption</h3>

Let Li6 be isotope A
Let Li7 be isotope B

<h3>How to determine whiche isotope is more abundant</h3>

Molar mass of isotope A (Li6) = 6.02 u
Molar mass of isotope B (Li7) = 7.02 u
Atomic mass of lithium = 6.94 u
Abundance of A = A%
Abundance of B = (100 - A)%

Atomic mass = [(mass of A × A%) / 100] + [(mass of B × B%) / 100]

6.94 = [(6.02 × A%) / 100] + [(7.02 × (100 - A)) / 100]

6.94 = [6.02A% / 100] + [702 - 7.02A% / 100]

6.94 = [6.02A% + 702 - 7.02A%] / 100

Cross multiply

6.02A% + 702 - 7.02A% = 6.94 × 100

6.02A% + 702 - 7.02A% = 694

Collect like terms

6.02A% - 7.02A% = 694 - 702

-A% = -8

A% = 8%

Thus,

Abundance of B = (100 - A)%

Abundance of B = (100 - 8)%

Abundance of B = 92%

SUMMARY

Abundance of A (Li6) = 8%
Abundance of B (Li7) = 92%

From the above, isotope Li7 is more abundant.

Learn more about isotope:

brainly.com/question/24311846

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2 years ago

A 256 mL sample of HCl gas is in a flask where it exerts a force (pressure) of 67.5 mmHg. What is the pressure of the gas if it

Effectus [21]

Answer:

The pressure in the new flask would be $128\; \rm mmHg$ if the $\rm HCl$ here acts like an ideal gas.

Explanation:

Assume that the $\rm HCl$ sample here acts like an ideal gas. By Boyle's Law, the pressure $P$ of the gas should be inversely proportional to its volume $V$ .

For example, let the initial volume and pressure of the sample be $V_1$ and $P_1$ . The new volume $V_2$ and pressure $P_2$ of this sample shall satisfy the equation: $P_1 \cdot V_1 =P_2 \cdot V_2$ .

In this question,

The initial volume of the gas is $V_1= 256\; \rm mL$ .
The initial pressure of the gas is $P_1 = 67.5\; \rm mmHg$ .
The new volume of the gas is $V_2 = 135\; \rm mL$ .

The goal is to find the new pressure of this gas, $P_2$ .

Assume that this sample is indeed an ideal gas. Then the equation $P_1 \cdot V_1 =P_2 \cdot V_2$ should still hold. Rearrange the equation to separate the unknown, $P_2$ . Note: make sure that the units for $V_1$ and $V_2$ are the same before evaluating. That way, the unit of

$\begin{aligned} & P_2\\ &= \frac{P_1 \cdot V_1}{V_2} \\ &= \frac{256\; \rm mL \times 67.5\; \rm mmHg}{135\; \rm mL} \\ & \approx 128\; \rm mmHg\end{aligned}$ .

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vagabundo [1.1K]

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