Q1) Which element is reduced in this reaction? 2Cr(OH)3+3OCl?+4OH??2CrO4?2+3Cl?+

Question

Q1) Which element is reduced in this reaction?

2Cr(OH)3+3OCl?+4OH??2CrO4?2+3Cl?+5H2O (enter chemical symbol of the element)

Q4) Three gases (8.00g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-Lcontainer. At 23.0 ?C, the total pressure in the container is 5.30 atm . Calculate the partial pressure of each gas in the container.(Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane.)

Part B

A gaseous mixture of O2 and N2 contains 40.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 585 mmHg ?

Express you answer numerically in millimeters of mercury.

Explanation / Answer

ANSWER.

Q1).Cl(chlorine).

Q2).Given data, volume=11.5x12x10ft=1380 cft=1380x28.2=38916.00 lt. pressure=1 atm.T=273+20=293K, R=0.0821it.atm/K. for ideal gas PV=nRT n=PV/RT------(1) substitute values in eq 1 n=(1x38916.00)/(0.0821x293) n=1617.5 moles as we know 1 mole always contains N(avagadro number) molecules so,1617.5 moles contains 1617.5xN molecules.i.e1617.5x6.023x1023. Q3)Given data,P=1.100(total pressure) atm,V=1L,T=273+25=298 K,n=1.1/39.948=0.28. preessure of argon=nRT/V---------(2)    substitute values in eq 2 par=(0.23x0.0821x298)/1=0.674atm. partial pressure of ethane=total pressure-par=1.10-0.674=0.426atm. Q4) Given data,P=5.3 atm,V=10.0L,T=296 K.   substitute values in eq 1.n=(5.3x10)/(0.0821x296)=2.18 moles. partial pressure of methane pm=mole fraction xtotal pressure=(0.50x5.3)/2.18=1.22 atm partial pressure of ethane pe=0.60x5.3/2.18=1.46 atm    partial pressure of propane=total pressure-(pm+pe)=5.3-2.68=2.62 atm=pp pm=1.22 atm    pe=1.46 atm  pp=2.62 atm. PART B

Given data,mass of nitrogen=40.8 gm, mass of oxygen gas=59.2 gm. molesof nitrogen=40.8/28=1.46, moles of oxygen=59.2/32=1.85. partial pressure of oxygen=molefraction x total pressure=(1.85/3.31)x585=0.56x585=326.96 mm ofHg.   partial pressure of oxygen=326.96mmHg.

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