At 570. mm hg and 25°c, a gas sample ne (in mm hg) at a volume of 1250 ml and a temperature of 175°c and 25°c, a gas sample has a volume of 2270 ml. what is the final pressure

final pressure ( P2) = 467.37 mm Hg

Explanation:

ideal gas:

∴ P1 = 570 mm Hg * ( atm / 760 mm Hg ) = 0.75 atm

∴ T1 = 25 ° C = 298 K

∴ V1 = 1.250 L

∴ R = 0.082 atm L / K mol

⇒ n = P1*V1 / R*T1

⇒ n = (( 0.75 ) * ( 1.25 )) / (( 0.082 ) * ( 298 ))

⇒ n = 0.038 mol gas

∴ T2 = 175 °C ( 448 K )

∴ V2 = 2.270 L

⇒ P2 = nRT2 / V2

⇒ P2 = (( 0.038 ) * ( 0.082 ) * ( 448 )) / 2.270

⇒ P2 = 0.615 atm * ( 760 mm Hg / atm ) = 467.37 mm Hg

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.  

answer; talc and gypsum;