Agas sample has an initial pressure of 547 mmhg and an initial volume of 0.500 l. what is the pressure (in atm) if you decrease the volume of the sample to 225 ml?

To solve this, we assume that the gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

P1V1 =P2V2

P2 = P1 x V1 / V2

P2 = 547 mmHg x 500 mL / 225 mL

P2 =1215.56 mmHg

1215.56 mmHg ( 1 atm / 760 mmHg) = 1.60 atm

Therefore, the new pressure of the gas would be 1.60 atm.

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