Answer:
=2h20−2kmno4+2mno2+2ckl+cl2+4hko+o2
Explanation:
step-by-step.
2mno2+4koh+o2+cl2−2kmno4+2kcl+2h20
=2mno2+4hko+o2+cl2+−2kmno4+2ckl+2h20
The correct answer to this question is this one:
use PV=nRT
we can convert it into P=(mRT/MV) then P=dRT/M
so at STP:
T= 25 celsius which equals 298.73 Kelvin
<span />d= 1.046 g/mL = 0.001046 g/L (we need to use litres in the ideal gas equation)
<span />R =0.08206 Latm/Kmol
<span />M= molar mass of C16H22O4, which is (12)16+(1)22+(16)4 = 278 g/mol
<span>so plug this into: P=dRT/M
once you found the pressure, P, you need to convert it into torr (because it will be in atm (atmospheres).. since 1 atm = 760 torr = 760 mm Hg
multiply P by 760 and you're done. You;ll have the pressure in torr </span>
Answer:
<h2>2.7 g/cm³</h2>
Explanation:
The density of a substance can be found by using the formula
From the question we have
We have the final answer as
<h3>2.7 g/cm³</h3>
Hope this helps you