CHEMISTRY HIGH SCHOOL

A mixture of two gases has a total pressure of 5.7 atm . If one gas has a partial pressure of 4.1 atm , what if the partial pressure of the other gas ?

Answers

Answer 1

Answer:

Answer:

1.6 atm

Explanation:

We are given that total pressure of mixture of two gases=5.7 atm

Partial pressure of one gas=4.1 atm

We have to find the partial pressure of other branch.

We know that Dalton;s law of partial pressure

It states that pressure exerted by mixture of gases is equal to sum of partial pressure exerted by gases in mixture.

Let x bet the pressure exert by other gas

Apply this law

Total pressure=4.1+x

$5.7=4.1+x$

$x=5.7-4.1=1.6$

Hence, the partial pressure of other gas=1.6 atm.

Answer 2

Answer: if the two gases has a total pressure of 5.7 atm and one of the gases has a partial pressure of 4.1 the the other one has the pressure of 1.6

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How are regional climate patterns caused by atmospheric and ocean flows

Answers

Answer:

Ocean currents act as conveyer belts of warm and cold water, sending heat toward the polar regions and helping tropical areas cool off, thus influencing both weather and climate. .

A snake slithers up a giant sand dune at 2 meters per second.How far will it have moved in a minute?

Answers

it will have traveled 120 metets

Answer:

A. 120m

Explanation:

just took the test

Bromine has two isotopes 79Br and 81Br, whose masses (78.9183 and 80.9163 amu) and abundances (50.69% and 49.31%, respectively) were determined in earlier experiments. Calculate the average atomic mass of bromine based on these experiments.

Answers

Answer:

Average atomic mass = 79.9034 amu

Explanation:

The formula for the calculation of the average atomic mass is:

$Average\ atomic\ mass=(\frac {\%\ of\ the\ first\ isotope}{100}* {Mass\ of\ the\ first\ isotope})+(\frac {\%\ of\ the\ second\ isotope}{100}* {Mass\ of\ the\ second\ isotope})$

Given that:

For first isotope:

% = 50.69 %

Mass = 78.9183 amu

For second isotope:

% = 49.31 %

Mass = 80.9163 amu

Thus,

$Average\ atomic\ mass=(50.69)/(100)* {78.9183}+(49.31)/(100)* {80.9163}\ amu$

$Average\ atomic\ mass=40.0036+39.8998\ amu$

Average atomic mass = 79.9034 amu

A gas at 255 kilopascals and 45°C has an initial volume of 2.00L. The pressure of the gas increases to 805 kilopascals as the temperature is raised to 255°C. What will be the new volume?1.05 liters
2.28 liters
1.25 liters
0.44 liters
1.50 liters

Answers

Answer : The correct option is, (a) 1.05 liters

Solution :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

$(P_1V_1)/(T_1)=(P_2V_2)/(T_2)$

where,

$P_1$ = initial pressure of gas = 255 kpa

$P_2$ = final pressure of gas = 805 kpa

$V_1$ = initial volume of gas = 2 L

$V_2$ = final volume of gas = ?

$T_1$ = initial temperature of gas = $45^oC=273+45=318K$

$T_2$ = final temperature of gas = $255^oC=273+255=528K$

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

$(255kpa* 2L)/(318K)=(805kpa* V_2)/(528K)$

$V_2=1.05L$

Therefore, the final or new volume of gas will be, 1.05 liters

Which of the following is a measure of randomness in a system?A) entropy.
B) kinetic energy.
C) potential energy.
D) chemical energy.

Answers

Answer:

A) entropy

Explanation:

Under which conditions of temperature and pressure does a sample of neon behave most like an ideal gas?(1) 100 K and 0.25 atm
(2) 100 K and 25 atm
(3) 400 K and 0.25 atm
(4) 400 K and 25 atm

Answers

Answer : The correct option is, (3) 400 K and 0.25 atm

Explanation :

The conditions for ideal gas are :

Ideal gas are those gas that has no intermolecular attractions.

Ideal gas are those gas that have negligible volume.

The ideal gas equation is,

$PV=nRT$

The conditions for real gas are :

Real gas are those gas that have intermolecular attractions.

Real gas are those gas that have volume.

The real gas equation is,

$(P+(an^2)/(V^2))(V-nb)=nRT$

A real gas behave ideally at high temperature and low pressure condition.

From the given options, option (3) have high temperature and low pressure is the correct option.

Hence, the 400 K and 0.25 atm conditions of temperature and pressure does a sample of neon behave most like an ideal gas.

Since real gases behave least ideally at low temperature and high pressure, they would behave most like an ideal gas at high temperature and low pressure.
Therefore, (3) 400K and 0.25 atm is the correct answer.
Hope this would help~

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