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choli [55]
3 years ago
6

A container holds 6.4 moles of gas. hydrogen gas makes up 25% of the total moles in the container. if the total pressure is 1.24

atm
Chemistry
2 answers:
klio [65]3 years ago
6 0
The total pressure of the mixture of gases is equal to the sum of the pressure of each gas as if it is alone in the container. The partial pressure of a component of the mixture is said to be equal to the product of the total pressure and the mole fraction of the component in the mixture.

Partial pressure of hydrogen gas = 1.24 atm x .25 = 0.31 atm
Partial pressure of the remaining = 1.24 atm x (1-.25) = 0.93 atm 
Vlad1618 [11]3 years ago
5 0

Answer:

0.31

Explanation:

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Larry bought 12 1/2 pounds of candy to share with his friends. If he gave each friend 2 1/2 pounds of candy, how many friends di
arlik [135]

Answer:

The answer to your question is: 5 friends

Explanation:

Data

Larry bought 12 1/2 pounds of candy

gave each friend 2 1/2 pounds

number of friends = ?

Process

Convert mixed fractions into improper fractions

           12 1/2 = (24 + 1) / 2 = 25 /2

            2 1/2 = (4 + 1) / 2 = 5/2

Divide the fractions

                                \frac{25}{2}  / \frac{5}{2}

                                = \frac{50}{10}

                               = 5

Larry gave candies to 5 of his friends

4 0
3 years ago
How many protons neutrons and electrons does beryllium have
choli [55]
Beryllium has 4 protons, 4 electrons and 5 neutrons
5 0
3 years ago
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Two gas-containers, A and B, are connected with a valve. The first container, A, has a volume of 135 mL, and the second containe
stiv31 [10]

Answer:

85.5 mmHg is the pressure of the gas sample when the valve is opened.

Explanation:

The combined gas equation is,

\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}

where,

P_1 = initial pressure of gas in container A = 165 mmHg

P_2 = final pressure of gas = ?

V_1 = initial volume of gas in container A= 135 mL

V_2 = final volume of gas = 135 mL + 117 mL = 252 mL

T_1 = initial temperature of gas in container A = 22.5^oC=273+22.5=295.5 K

T_2 = final temperature of gas = 12.7^oC=273+12.7=285.7K

Now put all the given values in the above equation, we get:

P_2=\frac{P_1V_1\times T_2}{T_1\times V_2}

=\frac{165 mmHg\times 135 mL\times 285.7 K}{295.5 K\times 252 mL}

P_2=85.5 mmHg

85.5 mmHg is the pressure of the gas sample when the valve is opened.

8 0
4 years ago
6. Calculate the molecular mass of acetylsalicylic acid (HOOC-C6H4-OOCCH3).
SVEN [57.7K]

Answer:

180.1574 g/mol

Explanation:

https://www.webqc.org/periodictable-Hydrogen-H.html

5 0
4 years ago
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Answer:

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