A 48.5 mL sample of gas in a cylinder is warmed from 18°C to 92°C.

What is its volume at the final temperature? (Assume constant pressure.)
Express your answer in milliliters to three significant figures.

60.8 mL

Explanation:

Using Charles law equation;

V1/T1 = V2/T2

Where;

V1 = initial volume (mL)

V2 = final volume (mL)

T1 = initial temperature (K)

T2 = final temperature (K)

According to the information given in this question;

V1 = 48.5 mL

V2 = ?

T1 = 18°C = 18 + 273 = 291K

T2 = 92°C = 92 + 273 = 365K

Using V1/T1 = V2/T2

48.5/291 = V2/365

Cross multiply

291 × V2 = 48.5 × 365

291 V2 = 17702.5

V2 = 17702.5 ÷ 291

V2 = 60.8 mL

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.