If 4.50 g of methane gas (CH4) is in a 2.00-L container at 35°C, what is the pressure in the
container?

The answer to your question is Pressure = 3.55 atm

Explanation:

Data

R = 0.082 atm L/mol°K

mass = 4.5 g

volume = 2 L

temperature = 35°C

Pressure = ?

Process

1.- Calculate the moles of Methane

molar weight = 12 + 4 = 16 g

                          16 g of Methane 1 mol

                          4.5 g                     x

                           x = (4.5 x 1)/16

                           x = 0.281 moles

2.- Convert temperature to Kelvin

°K = 273 + 35

    = 308

3.- Use the ideal gas law to solve this problem

          PV = nRT

- Solve for P

           P = nRT / V

- Substitution

           P = (0.281)(0.082)(308) / 2

- Simplification

           P = 7.097 / 2

- Result

            P = 3.55 atm

The pressure in the container is 3.55 atm

Explanation:

Step 1: Data given

Mass of methane gas = 4.50 grams

Volume = 2.00 L

Temperature = 35 °C = 308 K

Molar mass CH4 = 16.04 g/mol

Step 2: Calculate moles CH4

Moles CH4 = mass CH4 / molar mass CH4

Moles CH4 = 4.50 grams / 16.04 g/mol

Moles CH4 = 0.281 moles

Step 3: Calculate pressure

p*V = n*R*T

⇒with p = the pressure in the container = TO BE DETERMINED

⇒with V = the volume of the container = 2.00L

⇒with n = the moles of methane = 0.281 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒ T = the temperature = 308 K

p = (n*R*T)/V

p = (0.281 * 0.08206 * 308 ) / 2.00

p = 3.55 atm

The pressure in the container is 3.55 atm

answer is: nuclear fusion produces elements that are heavier than helium.

nuclei combine to form a heavier nucleus, releasing energy.  

for example, fusion of hydrogen atoms at the sun.  

this fusion nuclear reaction is in the inner core of the sun and hydrogen (atomic number 1) is conveted into helium (atomic number 2).  

the inner core is the central region of the sun and all solar energy is produced in the core by nuclear fusion.