A 500 ml sample of a gas was found to have a pressure of 1.0 atm at 25 degree C.

Question

A 500 ml sample of a gas was found to have a pressure of 1.0 atm at 25 degree C. What will be the new volume if the temperature is change to 50 degree C ar constant pressure. A 2.00 L sample of Nitrogen at 25.0 degree C was found have a pressure of 1.00 atm. How many moles of gas are present and what is the mass of the gas in grams? The total pressure in a mixture of Nitrogen and Chlorine gas was found to be 1.65 atm. if the partial pressure of Nitrogen was 0.65 atm, what is the partial pressure of chlorine gas. Octane, C_8H_18, is a flammable hydrocarbon. It undergoes a combustion reaction (with oxygen gas) to produce Carbon dioxide and water. Write a balanced chemical equation for this reaction How many mole of oxygen is consumed if 0.050 mol of Octane undergoes Combustion?

Explanation / Answer

Q8.

i)

V = 50 mL gas

P1 = 1 atm , T1 = 25°C

find new vol., V2 = ? if P is constant and T2 = 50°C

V1/T1 = V2/T2

50/(273+25) = V2/(50+273)

V2 = 50/(273+25)*(50+273)

V2 = 54.1946 mL

iii)

V = 2 L of N2, T = 25°C = 298K, P = 1 atm

P V= nRT

n = PV/(RT)

n = (1*2)/(0.082*298) = 0.0818464 mol of N2

mass = mol*MW = 0.0818464*28 = 2.291699 g of N2

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