A.) how many grams of NO2, nitrogen dioxide, are contained in 0.500L of the gas

Question

A.) how many grams of NO2, nitrogen dioxide, are contained in 0.500L of the gas at STP?

B.) Calculate the density of NO2 gas, in grams per liter, at 110`C and 12atm.

C.) Calculate the molar mass of a gas if 0.125g of the gas occupies 93.3 mL at STP.

D.) on a spring morning (15`C) you fill your tires to a pressure of 2.25 atmospheres. as you ride along, the tire heats up to 45`C from the friction on the road. what is the pressure in your tires now?

E.) What volume of H2 is formed at STP when 6.0g of Al is treated with excess NaOH? 2NaOH+2Al+6H2O-->2NaAl(Oh)4+3H2(g)

Explanation / Answer

PV= nRT

at STP T=298K

P= 101325Pa

R = 8.314 j/mol-K

(a) v= 0.5L = 0.0005m^3

n= PV/RT

n=0.0204 moles

(b) P= 12 atm = 1215900Pa

T= 110C = 383K

PV=nRT

PV= m/M *RT

PM=m/V *RT

PM = DRT

D=PM/RT

D = 17564.949 G/m^3 = 17.56g/L

(c) V= 93.3ml = 93.3*10^-6m^3

m = 0.125g

M= mRT/PV

M= 32.76g/mol

(d) V,R,n remain constant so

T1/T2 = P1/P2

p2 = 15/45*2.25 = 6.75atm

(e) m=6g

moles of al = 6/27 = 0.222 moles

2mole of Al produce 3 moles of H2

so 0.222moles produce 0.333moles H2

V=nRT/P

V = 8.14*10^-3 m^3 = 8.14L

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