1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
vaieri [72.5K]
3 years ago
5

Hydrogen gas is filled in a 224 ml glass container at 0 degree celcius and 1 atmospheric pressure. What are the number of molecu

le of hydrogen in the container??
Chemistry
2 answers:
Step2247 [10]3 years ago
8 0

Answer:

\boxed{\text{6.02 $\math{\times 10^{21}}$ molecules}}

Explanation:

A pressure of 1 atm and a temperature of 0 °C is the old definition of STP. Under these conditions, 1 mol of a gas occupies 22.4 L.

1. Calculate the moles of hydrogen.

n = \text{0.224 L} \times \dfrac{\text{1 mol}}{\text{22.4 L}} = \text{0.0100 mol}

2. Calculate the number of molecules

\text{No. of molecules} = \text{0.0100 mol} \times \dfrac{\text{6.022 $\times 10^{23}$ molecules}}{\text{1 mol}}\\\\= \textbf{6.02 $\mathbf{\times 10^{21}}$ molecules}\\\\\text{The sample contains }\boxed{\textbf{6.02 $\mathbf{\times 10^{21}}$ molecules}}

vfiekz [6]3 years ago
4 0

Answer:  6.02 × 10^{21} molecules of hydrogen are in the container. The Ideal Gas Law equation gives the relationship among the pressure, volume, temperature, and moles of gas.  Once the moles of gas is determined, we use Avogadro's number, 6.022 × 10^{23} to get he number of molecules.

Further Explanation:

The Ideal Gas Equation is:  

PV = nRT  

where:  

P - pressure (in atm)  

V - volume (in L)  

n - amount of gas (in moles)  

R - universal gas constant 0.08206 \frac{L-atm}{mol-K}  

T - temperature (in K)  

In the problem, we are given the values:  

P = 1 atm  

V = 224 mL  = 0.224 L (3 significant figures)

n = ?

T = 0 degrees Celsius

We need to convert the temperature to Kelvin before we can use the Ideal Gas Equation. The formula to convert from degree Celsius to Kelvin is:  

Temperature \ in \ Kelvin = Temperature\ in \ Celsius \ + \ 273.15  

Therefore, for this problem,  

Temperature\ in \ K = 0 +273.15\\Temperature\ in \ K = 273.15  

Solving for n using the Ideal Gas Equation:  

n \ = \frac{PV}{RT}\\n \ = \frac{(1 \ atm) \ (0.224 \ L)}{(0.08206 \ \frac{L-atm}{mol-K})( 273.15 \ K)} \\ n \ = 9.99\ X \ 10^{-3} mol

Now that we know the number of moles of hydrogen gas, we can determine how many molecules there are:

no.\ of \ molecules \ = moles \ of \ hydrogen \ (\frac{6.022 \ X \ 10^{23} molecules}{1 \ mole\ of \ hydrogen} )\\no.\ of \ molecules \ = 9.99 \ X \ 10^{-3} \ moles \ (\frac{6.022 \ X \ 10^{23} molecules}{1 \ mole\ of \ hydrogen} )\\ no. \ of \ molecules \ = 6.02 \ X 10^{21} \ molecules \ of \ hydrogen

Learn More  

1. Learn more about Boyle's Law brainly.com/question/1437490  

2. Learn more about Charles' Law brainly.com/question/1421697  

3. Learn more about Gay-Lussac's Law brainly.com/question/6534668  

Keywords: Ideal Gas Law, Volume, Pressure  

You might be interested in
I need help with science pls​
Vinvika [58]

Answer: i honestly dont know that is like what 9th grade science im only a 6th grader lol

Explanation: none

7 0
2 years ago
The Henry's law constant for helium gas in water at 30 °C is 3.70 × 10-4 M/atm. When the partial pressure of helium above a samp
igor_vitrenko [27]

Answer:

The concentration of helium in the water is 2.405×10^-4 M

Explanation:

Concentration = Henry's law constant × partial pressure of helium

Henry's law constant = 3.7×10^-4 M/atm

Partial pressure of helium = 0.65 atm

Concentration = 3.7×10^-4 × 0.65 = 2.405×10^-4 M

4 0
3 years ago
Which of the following must be true about a reaction if it is only spontaneous at high temperatures?
Neporo4naja [7]
The correct answer is B, 
<span>It is endothermic, with both positive enthalpy and entropy changes.</span>
4 0
2 years ago
How many grams of Na2SO4 should be weighed out to prepare 0.5L of a 0.100M solution?​
Nezavi [6.7K]

Answer:

7 gram of Na2SO4 should be required to prepare 0.5L of a 0.100 M solution.

Explanation:

First of all the molecular weight of Na2SO4 is 142.08 gram.Now we all know that if the molecular weight of a compound is dissolved in 1000ml or 1 litee of water then the strength of that solution becomes 1 M.

    According to the given question we have to prepare 0.100 M solution

1000 ml of solution contain 142.08×0.1= 14.208 gram Na2SO4

1    ml of solution contain     14.208÷1000= 0.014 gram

0.5L or 500ml of solution contain 0.014×500= 7gram Na2SO4.

 So it can be stated that 7 gram of Na2SO4 should be required to prepare 0.5L of a 0.100M solution.

     

3 0
2 years ago
4. which answer below is the formula mass of a water molecule?
mars1129 [50]
The answer is 18.02 g/mol
6 0
3 years ago
Other questions:
  • Animals and plants need to maintain homeostasis to function properly.<br><br> A)True<br> B)False
    15·2 answers
  • Two atoms that are isotopes of one another must have the same number of what? Question 6 options: protons all particles atomic m
    7·2 answers
  • These two beakers represent solutions of HCl and NaOH. Describe a third beaker showing the ions that remain after the reaction h
    15·1 answer
  • What are the correct answers to these questions?
    15·1 answer
  • Compared to a solid, the molecular bonds of a liquid are.
    12·2 answers
  • Please help what are the number atoms for each?!
    12·1 answer
  • Which of the pairs below would be the best choice for a pH 5 buffer? HF/NaF, K a (HF) = 3.5 × 10-4 HC2H3O2/KC2H3O2, K a (HC2H3O2
    13·1 answer
  • The pKa of a solution is defined by the equation pKa=-log Ka
    10·1 answer
  • I need help writing a LAB REPORT about NATURAL SELECTION
    12·1 answer
  • A
    8·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!