80.0 ML of fluorine gas is held in a flexible vessel at STP. If the vessel is transported to the surface of Venus where the pressure is 92.0 ATM and The temperature is 460 Celsius what is the new volume of the gas in millimeters

The new volume of the gas is 2.33 mL

Explanation:

Step 1: data given

Volume of the fluorine gas = 80.0 mL = 0.080 L

STP = 1 atm and 273 K

The new pressure is 92.0 atm

The new temperature = 460 °C = 733 K

Step 2: Calculate the new volume

P1*V1 / T1  = P2 *V2 / T2

⇒with P1 = the initial pressure of the fluorine gas = 1 atm

⇒with V1 = the initial volume of the fluorine gas = 0.080 L

⇒with T1 = the initial temperature of the fluorine gas = 273 K

⇒with P2 = the new pressure of the gas = 92.0 atm

⇒with V2 = the new volume of the gas = TO BE DETERMINED

⇒with T2 = the new temperature of the gass = 733 K

(1 atm * 0.080 L)/273 K = (92.0 atm * V2) / 733 K

2.93 * 10^-4 = (92.0 atm * V2) / 733 K

0.214769 = (92.0 atm * V2)

V2 = 0.214769 / 92.0

V2 = 0.00233 L = 2.33 mL

The new volume of the gas is 2.33 mL

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g

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