A sample of sulfur dioxide (SO2) is initially at a temperature of 133 C a volume of 20 L, and a pressure of 850 mm Hg. If the volume changes to 25 L and the temperature increases to 181 C, what is the new pressure?

Show your work. Don't forget to convert C to kelvin

760.39 mmHg (approx.)

Explanation:

Okay so given the first set of information, we have:

T = 406 K (133+273)

V = 20 L

P = 1.1184 atm (converted for continuity reasons from mmHg)

R = 0.08206 L atm/mol K

Using PV = nRT (ideal gas law), we solve for n (moles of SO2).

n = PV/RT = (1.1184 atm * 20 L) / (0.08206 L atm/mol K * 406 K) = 0.6714 mol

Now that you have all the information, you can use the new volume and temperature to solve for pressure.

T = 454 K (181+273)

V = 25 L

n = 0.6714 mol

R = 0.08206 L atm/mol K

Using the ideal gas law again, we solve for P (pressure in atm).

P = nRT/V = (0.6714 mol * 0.08206 L atm/mol K * 454 K) / (25 L) = 1.0005 atm

Then we convert atm back to mmHg to get 760.39 mmHg.

answer: c.

explanation:

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6