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Vilka [71]
2 years ago
9

A mouse is placed in a sealed chamber with air at 769.0 torr. This chamber is equipped with enough solid KOH to absorb any CO2 a

nd H2O produced by the mouse. The gas volume in this chamber is measured to be exactly 2.20 L, the temperature is held constant at 292 K. After two hours the pressure inside the bottle falls to 717.1 torr. What mass of oxygen has the mouse consumed?
Chemistry
1 answer:
svlad2 [7]2 years ago
5 0

<u>Answer:</u> The amount of oxygen gas consumed by mouse is 0.202 grams.

<u>Explanation:</u>

We are given:

Initial pressure of air = 769.0 torr

Final pressure of air = 717.1 torr

Pressure of oxygen = Pressure decreased = Initial pressure - Final pressure = (769.0 - 717.1) torr = 51.9 torr

To calculate the amount of oxygen gas consumed, we use the equation given by ideal gas which follows:

PV=nRT

where,

P = pressure of the gas = 51.9 torr

V = Volume of the gas = 2.20 L

T = Temperature of the gas = 292 K

R = Gas constant = 62.364\text{ L. Torr }mol^{-1}K^{-1}

n = number of moles of oxygen gas = ?

Putting values in above equation, we get:

51.9torr\times 2.20L=n\times 62.364\text{ L. Torr }mol^{-1}K^{-1}\times 292K\\\\n=\frac{51.9\times 2.20}{62.364\times 292}=0.0063mol

To calculate the mass from given number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of oxygen gas = 0.0063 moles

Molar mass of oxygen gas = 32 g/mol

Putting values in above equation, we get:

0.0063mol=\frac{\text{Mass of oxygen gas}}{32g/mol}\\\\\text{Mass of oxygen gas}=(0.0063mol\times 32g/mol)=0.202g

Hence, the amount of oxygen gas consumed by mouse is 0.202 grams.

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An ionic compound is formed between a metal and a non metal. The metal being electropositive can form a cation by transferring the electron to the electronegative non metal that gains the electrons to form an anion. Both the elements try to get a stable octet configuration by the transfer of electrons. The number of electrons lost by metal will be equal to the number of electrons gained by the non metal. Hence, the magnitude of positive charge on the cation will be equal to the magnitude of negative charge on the anion. Therefore, the overall charge on the compound will be 0

So the correct answer is the sum of all charges in the formula for an ionic compound is 0

5 0
3 years ago
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Under what conditions is the change in internal energy, δe rxn , equal to the heat evolved in a chemical reaction?
Stells [14]
 the first law says that  the change in internal energy of a system is given by: 

δ<span>E = δq + δw</span>

where δ<span>E is the i change in internal energy, </span>

<span>δq is the amount of thermal energy added to the system from the surroundings </span>

<span>δw is the l work done *on* the system *by* the surroundings. </span>

<span>For a system only undergoing expansion work,
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δE = δq - p δ<span>V </span>
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4 0
2 years ago
A certain reaction has an activation energy of 39.5 kJ/mol. As the temperature is increased from 25.0°C to a higher temperature,
riadik2000 [5.3K]

Answer:

Explanation:

We shall apply Arrhenius equation which is given below .

ln\frac{k_2}{k_1} = \frac{E_a}{R} [\frac{1}{T_1} -\frac{1}{T_2} ]

K₂ and K₁ are rate constant at temperature T₂ and T₁ , Ea is activation energy .

Putting the given values

ln\frac{5.9}{1} = \frac{39500}{8.3} [\frac{1}{298} -\frac{1}{T_2} ]

.000373= [\frac{1}{298} -\frac{1}{T_2} ]

T₂ = 335.27 K

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4 0
3 years ago
The natural gas in a storage reservoir, under a pressure of 1.00 atmosphere, has a volume of 2.74 × 109 L at 20.0°C. The tempera
Soloha48 [4]

Answer : The final volume of gas will be, 2.36\times 10^9L

Explanation :

Charles' Law : It is defined as the volume of gas is directly proportional to the temperature of the gas at constant pressure and number of moles.

V\propto T

or,

\frac{V_1}{V_2}=\frac{T_1}{T_2}

where,

V_1 = initial volume of gas = 2.74\times 10^9L

V_2 = final volume of gas = ?

T_1 = initial temperature of gas = 20.0^oC=273+20.0=293K

T_2 = final temperature of gas = -20.0^oC=273+(-20.0)=253K

Now put all the given values in the above formula, we get the final volume of the gas.

\frac{2.74\times 10^9L}{V_2}=\frac{293K}{253K}

V_2=2.36\times 10^9L

Therefore, the final volume of gas will be, 2.36\times 10^9L

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3 years ago
What is the answer please help
snow_lady [41]

Answer:

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Explanation:

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