States of Matter - Online Test
Q1.
What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 flask at ?
Answer : Option C
Explaination / Solution:
P=P1+P2 (Acc. To Daltons Law) And P1×9=0.2xRT And P2×9=0.1xRT where T= 300K
Q2. What will be the pressure of the gaseous mixture when 0.5 L of at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at?
Answer : Option C
Explaination / Solution:
x1=0.8x0.5 x 1=0.7x2 And P=+
Q3. Density of a gas is found to be 5.46 at 27 at 2 bar pressure. What will be its density at STP?
Answer : Option A
Explaination / Solution:
3g/
Q4. 34.05 mL of phosphorus vapour weighs 0.0625 g at 546 and 0.1 bar pressure. What is the molar mass of phosphorus?
Answer : Option B
Explaination / Solution:
PV=(0.0625/M)RT where p=0.1bar T=819.15K and V= 34.05ml
Q5.
A student forgot to add the reaction mixture to the round bottomed flask at 27 but instead he/she placed the flask on the flame. After a lapse of time, he realized his mistake, and using a pyrometer he found the temperature of the flask was 477 . What fraction of air would have been expelled out?
Answer : Option A
Explaination / Solution:
n1/n2=T2/T1 =0.4 so fraction of air expelled out =1-0.6=0.4.
Q6. Calculate the temperature of 4.0 mol of a gas occupying 5 at 3.32 bar. (R = 0.083 bar ).
Answer : Option A
Explaination / Solution:
wehavePV=nRTorT=PVnR=3.22bar×5dm34mol×0.083bardm3K−1mol−1=50K
Q7. Calculate the total number of electrons present in 1.4 g of dinitrogen gas.
Answer : Option C
Explaination / Solution:
molesofN2=1.428=0.05molAnd1moleofN2=6.022×1023moleculesofN2And1moleculeofN2has14electronstotalnumberofelectronsin1.4gofN2=0.5×6.022×1023×14=4.214×1023
Q8. The van der Waals Equation adjusts the measured volume
Answer : Option A
Explaination / Solution:
nb is subtracted.
Q9. The van der Waals Equation adjusts the measured pressure
Answer : Option B
Explaination / Solution:
/ is added.
Q10.
Pay load is defined as the difference between the mass of displaced air and the mass of the balloon. Calculate the pay load when a balloon of radius 10 m, mass 100 kg is filled with helium at 1.66 bar at. (Density of air = 1.2 kg m-3 and R = 0.083 bar .
Answer : Option B
Explaination / Solution:
Volume of balloon,V=4/3(3.14) =4187 Mass of displaced air,m=V × δ =4187 x 1.2=5024.4 kg Temperature,T=300 K Moles of gas present,n=PV/RT=279.1 × 103 moles Mass of helium=279.1 ×103 x 4=116.4 kg Mass of filled balloon,m'=100+1116.4=1216.4 kg Payload=m-m'=3811.1 kg
