Question

D Question 47 5 pts A gas sample is at 338 Kwith a pressure of 1.26 atm. The molar mass of the gas is 44.01 g/mol. What is the density of gas? Report your answer to the nearest whole number and do NOT include units in your answer, only type in the number. Question 48 Consider the balanced chemical equation: 5 pts 4HSICS) – SIH_(g) + 3 SICIAN How many mol of SiCare produced for every 29 mol of HSC131) consumed? Report your answer to the nearest whole number and do NOT include units in your answer, only type in the number.

Answer 1

47) PV=nRT

P=Pressure=1.26 atm, T=temperature=338 K ;R=0.0821 L atm K-1 mol-1,M=Molar mass is given by 44.01 g/mol

n=no of moles=given mass/Molar mass,let given mass be m,and Molar mass be M

PV=m*R*T/M ; d=density=given mass/Volume=m/V

P=[m*R*T/][M*V]

P=d *R*T/ M    (as m/V=d)

d= [P*M]/[R*T]=    [1.26 atm *44.01 g/mol]/[0.0821 L atm K-1 mol-1*338 K]

=1.998 g/L= 2 g/L

Answer= Density is

2

48) 4 HSiCl3(l) $\rightarrow$ SiH4(g)+3 SiCl4(l)

From the balanced equation 4 moles of HSiCl3 gives 3 moles of SiCl4

When 29 moles of HSiCl3 has been consumed   [3 moles of SiCl4][29 moles of HSiCl3]/[4 moles of HSiCl3]

=21.75 moles of SiCl4 has been produced=22 moles of SiCl4(to the nearest whole number)

Answer=

22