A 6.69 L cylinder contains 1.62 mol of gas A and 4.00 mol of gas B, at a temperature of 27.3 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior.

The partial pressure of gas A is 5.97 atm

The partial pressure of gas B is 14.73 atm

Explanation:

From the ideal gas equation

PV = nRT

P = nRT/V

n is total moles of gas mixture = 1.62 + 4 = 5.62 moles

R = 82.057×10^-3 L.atm/gmol.K

T = 27.3°C = 27.3+273 = 300.3 K

V = 6.69 L

P (total pressure in the cylinder) = 5.62×82.057×10^-3×300.3/6.69 = 20.7 atm

Partial pressure of gas A = 1.62/5.62 × 20.7 atm = 5.97 atm

Partial pressure of gas B = 4/5.62 × 20.7 atm = 14.73 atm

atomic = no of protons.

mass number-atomic number = neutron number

answer: the metamorphic rocks are formed when they are exposed to high pressure and high temperatures. this happens when one of the earth's plates comes in contact with the other plate by traveling in opposite directions, straight into each other or slipping under one another. the friction that is caused by this activity results in   melting of rocks and when it cools they are known as metamorphic rocks. this process needs a controlled amount of pressure and temperature otherwise it may turn into magma.