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marusya05 [52]
3 years ago
10

The volume of a gas is 450 mL when its pressure is 1.00 atm. If the temperature of the gas does not change, what is the pressure

when its volume is changed to 2.00 L?
Use: P1V1=P2V2

A) 0.225 atm
B) 0.444 atm
C) 2.25 atm
D) 4.44 atm
Chemistry
1 answer:
juin [17]3 years ago
6 0

Answer:

A) 0.225atm

Explanation:

P1V1 = P2V2

V1 = 450ml

P1 = 1.0atm

V2 = 2L = 2 X 100 = 2000ml

P2 =?

1.0 X 450 = P2 X 2000

P2 = (1.0 X 450)/2000

    = 0.225atm

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How many liters of 3.5 M solution can be made using 23 moles of LiBr *must show work to get credit*
MrMuchimi

<u>Answer:</u> 6.57 L of solution can be made.

<u>Explanation:</u>

Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:

\text{Molarity of solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (L)}} .....(1)

Given values:

Molarity of LiBr = 3.5 M

Moles of LiBr = 23 moles

Putting values in equation 1, we get:

3.5mol/L=\frac{23mol}{\text{Volume of solution}}\\\\\text{Volume of solution}=\frac{23mol}{3.5mol/L}=6.57L

Hence, 6.57 L of solution can be made.

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3 years ago
Al comenzar la reacción: N2(g) + 2O2(g) ------&gt; 2NO2(g) existe 1 mol de N2 y 2 moles de O2 y al
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Answer:

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2 years ago
Based on the chemical equation, use the drop-down menu to choose the coefficients that will balance the chemical equation:
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Alice and Bob are experimenting with two moles of neon, a monatomic gas, that starts out at conditions of standard temperature a
Archy [21]

Answer:

29273.178 joules have been added to the gas for the entire process.

Explanation:

The specific heats of monoatomic gases, measured in joules per mol-Kelvin, are represented by the following expressions:

Isochoric (Constant volume)

c_{v} = \frac{3}{2}\cdot R_{u} (1)

Isobaric (Constant pressure)

c_{p} = \frac{5}{2}\cdot R_{u} (2)

Where R_{u} is the ideal gas constant, measured in pascal-cubic meters per mol-Kelvin.

Under the assumption of ideal gas, we notice the following relationships:

1) Temperature is directly proportional to pressure.

2) Temperature is directly proportional to volume.

Now we proceed to find all required temperatures below:

(i) <em>Alice heats the gas at constant volume until its pressure is doubled</em>:

\frac{T_{2}}{T_{1}} = \frac{P_{2}}{P_{1}} (3)

(\frac{P_{2}}{P_{1}} = 2, T_{1} = 273.15\,K)

T_{2} = \frac{P_{2}}{P_{1}} \times T_{1}

T_{2} = 2\times 273.15\,K

T_{2} = 546.3\,K

(ii) <em>Bob further heats the gas at constant pressure until its volume is doubled</em>:

\frac{T_{3}}{T_{2}} =\frac{V_{3}}{V_{2}} (4)

(\frac{V_{3}}{V_{2}} = 2, T_{2} = 546.3\,K)

T_{3} = \frac{V_{3}}{V_{2}}\times T_{2}

T_{3} = 2\times 546.3\,K

T_{3} = 1092.6\,K

Finally, the heat added to the gas (Q), measured in joules, for the entire process is:

Q = n\cdot [c_{v}\cdot (T_{2}-T_{1})+c_{p}\cdot (T_{3}-T_{2})] (5)

If we know that R_{u} = 8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K}, n = 2\,mol, T_{1} = 273.15\,K, T_{2} = 546.3\,K and T_{3} = 1092.6\,K, the heat added to the gas for the entire process is:

c_{v} = \frac{3}{2}\cdot \left(8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K} \right)

c_{v} = 12.471\,\frac{J}{mol\cdot K}

c_{p} = \frac{5}{2}\cdot \left(8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K} \right)

c_{p} = 20.785\,\frac{J}{mol\cdot K}

Q = (2\,mol)\cdot \left[\left(12.471\,\frac{J}{mol\cdot K} \right)\cdot (536.3\,K-273.15\,K)+\left(20.785\,\frac{J}{mol\cdot K} \right)\cdot (1092.6\,K-546.3\,K )\right]

Q = 29273.178\,J

29273.178 joules have been added to the gas for the entire process.

6 0
2 years ago
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