Number 19 please 16. Given the mass of one mole of gaseous NO is 30.0 grams/mole
ID: 705200 • Letter: N
Question
Number 19 please 16. Given the mass of one mole of gaseous NO is 30.0 grams/mole calculate the density of NO in grams/liter at STP a. 1.12 g/L b. 0.987 g/lL c. 2.17 g/L 64.0 g of oxygen gas in a 1.50-L 17. What is the pressure of container at -37°C? a, 4.12 atm 8 atm c. $1.6 atm d. 19.6 atm e. 8.2 atm 18. What is the volume that 57.0 grams of F, would occupy at 227°C and 1.50 atm? a. 1.06 L b. 18.6L d.82.1 L e. 106 L 19. What is the volume occupied by 10.0 grams of NH, at 500.°C and 1140 torr? a. 14.9L b. 16.1 L e. 24.9 L d. 32.7L e. 46.2 L 20. How many moles of Argon would occupy 75 mL at 33°C and 1.07 atm? a" 3.19 3P010 d. 3.15010* e. 0.313
Explanation / Answer
From ideal gas equation
PV = n RT
V = n RT /P
Here
Amount of NH3 = 10 g
Moles of NH3 = amount in g / molar mass
= 10g /17.031 g/mol
=0.587 moles
Pressure = 1140 torr or 1140*1 atm /760= 1.5 atm
Temperature = 500 C = 773 K
Therefore
V = n RT /P
= 0.587* 0.08206 *773 /1.5
= 24.9 L
The correct answer is C
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