1.018 g of Freon-113 gas is trapped in a 145 mL container at 760 mmHg and 50.0 d

Question

1.018 g of Freon-113 gas is trapped in a 145 mL container at 760 mmHg and 50.0 degree C. What is the molar mass of Freon-113? 21.7 g/mol 28 8 g/mol 46.1 g/mol 186 g/mol 245 g/mol Gas A and gas B are combined in a flask at initial pressures of 1.0 atm each. The flask is sealed and over time they react to completion to give gas C according to the following chemical equation: 2A(g) + B(g) rightarrow C(g) Assuming the temperature stays constant, what will be the total pressure in the flask after the reaction goes to completion? 0.33 atm 0.50 atm 0.67 atm 0.75 atm 1.0 atm Deviations from the ideal gas law are greater at low temperatures and low pressures. low temperatures and high pressures. high temperatures and high pressures. high temperatures and low pressures. A spacecraft is filled with 0.500 atm of O_2 and 0.500 atm of He. If there is a very small hole in the side of this craft such that gas is lost slowly into outer space. He is lost 2 8 times faster than O_2 is lost. He is lost 8 times faster than O_2 is lost. He is lost twice as fast as O_2 is lost. O_2 is lost 2.8 times faster than He is lost. O_2 is lost 8 times faster than He is lost. Which of the following does not fit the definition of a Bronsted Acid? H_3PO_4 H_2PO_4^- H_2O NH_4^+ CO_2

Explanation / Answer

17)

we know that

for gases

PV = nRT

now

moles (n) = mass (m) / molar mass (M)

so

PV = mRT/M

PVM = mRT

so

given

P = 760 mm Hg = 1 atm

V = 145 ml = 0.145 L

R = 0.0821

T = 50 C = 50 + 273 = 323 K

m = 1.018

so

1 x 0.145 x M = 1.018 x 0.0821 x 323

M = 186

so

molar mass of freon is 186 g / mol

so

the answer is D) 186 g/mol

18)

initial pressures of A and B are 1 atom

so

according to PV = nRT

moles of A = moles of B = y

now

consider the given reaction

2A + B --> C

we can see that

moles of A required = 2 x moles of B = 2 x y = 2y

but only y moles of A is present

so

B is in excess and A is the limiting reagent

so

moles of B reacted = 0.5 x moles of A present = 0.5 x y = 0.5y

moles of A left = 0

moles of C formed = moles of B reacted = 0.5y

moles of B left = y - 0.5y = 0.5y

so

finally

total moles = moles of A left + moles of B left + moles of C formed

total moles = 0 + 0.5y + 0.5y = y

so

total pressure = 1 atm

so

the answer is E) 1 atm

19)

B) low temperatures and high pressures

20)

we know that

r1/r2 = sqrt (M2/M1)

so

rHe / r02 = sqrt ( molar mass of 02 / molar mass fo He)

rH2 / r02 = sqrt ( 32 / 4)

rH2/r02 = 2.828

rH2 = 2.828 x r02

so

He is lost 2.8 times faster than 02 is lost

so

the answer is option A

21)

we know that

a bronsted acid can donate a proton (H+)

from the list

H3P04 , H2P04- , H20 and NH4+ can donate a H+ ion

but

C02 cannot donate a H+ ion

so

C02 is not a bronsted acid

so

the answer is E) C02

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