Question

2. An unknown gas has a density of 0.714 g/L at STP. What is the molar mass of the unknown gas? 3. What is the molar mass of a gas if 0.891 liters at 20.0°C and 1.20 atm weighs 3.17 g? 4. Acetylene gas, CH2, reacts with oxygen gas to produce gaseous carbon dioxide and liquid water. Write the balanced equation for this reaction. What volume of CO2 is produced at STP from 5.00 g 02? 5. What is the density of CO2 gas on the surface of Venus, where typical conditions are 650°C at a pressure of 90. atm?

Answer 1

-002Q According to ideal gas law Z PV = nRT pa presure ; v= Volume = no. of moles ; R= gas constant I= Temperature, As - no. of moles = no. of given mass - w Molar massm 7 pu= wort 7 pm - WRT density (8t= mass = ♡ volyme v PM = LRT Here p- pressure ; M = molar mass f= clensity R=gos.Gongdant T= Temperative

- | At STP Condition) P- 7 am T=0°c = R13K R = 0.0821 L-alm Il moel and given that - 8= density = 0.114 gt' putting all value; we get 1 apo x M = 0.114.97 x 0.0841 Kammermoë' x 273 M = _0.714_X0.0821 XP73gmoer 3 m = 16.00 g moe This | Malax mass of Onknown gas = 16.00 gmode!