if 0.896 grams of a gas occupies a 250 ml flask at 20 degrees celcius and 760 mm hg of pressure,what is the molar mass of the gas?

Pv=nRT PV/RT=n. 1l=100ml x=250ml. 100x=250/100 ×=750//76 =10=1atm ×0.25l/0.082×293.15 =0.010400069. Answer=0.0104g

First, note the correct spelling of celsius.

UsePV = nRT and solve for n = number of mols, then n = grams/molar mass. You have g and n, solve for molar mass.

g= 45

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To find the molar mass of a gas, we can use the ideal gas law equation:

PV = nRT

Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant (0.0821 L*atm/(mol*K))
T = Temperature

First, let's convert the given pressure from millimeters of mercury (mmHg) to atmospheres (atm). We can use the conversion factor: 1 atm = 760 mmHg.

So, the pressure becomes:
P = 760 mmHg / 760 mmHg = 1 atm

Next, convert the volume from milliliters (ml) to liters (L):
V = 250 ml = 250/1000 L = 0.25 L

Now, let's substitute the values into the ideal gas law equation to find the number of moles (n):

1 * 0.25 = n * 0.0821 * (20 + 273)
0.25 = n * 0.0821 * 293
0.25 = n * 24.006

Solving for n:
n = 0.25 / 24.006
n ≈ 0.01041358 moles

Next, we'll calculate the molar mass of the gas. The molar mass is given by the formula:

Molar Mass = Mass / Moles

Given mass = 0.896 grams and moles ≈ 0.01041358 moles, we can calculate:

Molar Mass = 0.896 g / 0.01041358 mol
Molar Mass ≈ 86.05 g/mol

Therefore, the molar mass of the gas is approximately 86.05 g/mol.