Given 482 milliliters of a gas at 37 degrees Celsius and at 1.3 atmospheres, how many moles of gas are present? (The ideal gas constant is 0.0821 L · atm/mol · K.)

2.46 x 101 moles

2.06 x 100 moles

2.06 x 10-1 moles

2.46 x 10-2 moles

The number of moles gas = 2.46 *10^-2 moles

Explanation:

Step 1: Data given

Volume = 482 mL = 0.482 L

Temperature = 37 °C

Pressure = 1.3 atm

The gas constant = 0.08206 L*atm/mol*K

Step 2: Calculate the number of moles of gas

pV = nRT

⇒with p =the pressure of the gas = 1.3 atm

⇒with V = the volume of the gas = 0.482 L

⇒with n = the number of molesgas= TO BE DETERMINED

⇒with R = the gas constant = 0.0821 L*atm/mol*K

⇒with T = the temperature = 37°C = 310 K

n = (pV)/(RT)

n = (1.3*0.482)/(0.0821*310)

n= 0.0246 moles = 2.46 *10^-2 moles

The number of moles gas = 2.46 *10^-2 moles

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

fe 55.85 g/mol and h2o 18.02 g/mol.