What will the pressure be if 89.9 moles of argon are contained in a 12.0 L cylinder that is pressurized at a temperature of 300
1 answer:
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Answer:
p3=0.36atm (partial pressure of NOCl)
Explanation:
2 NO(g) + Cl2(g) ⇌ 2 NOCl(g) Kp = 51
lets assume the partial pressure of NO,Cl2 , and NOCl at eequilibrium are P1 , P2,and P3 respectively
p1=0.125atm;
p2=0.165atm;
p3=?
Kp=51;
On solving;
p3=0.36atm (partial pressure of NOCl)
Answer:
391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.
Explanation:
Density of the gasoline ,d= 0.692 g/mL
Volume of gasoline in an tanks,V = 22.0 gallons = 83,279.02 mL
Let mass of the gasoline be M
M = V × d = 83,279.02 mL × 0.692 g/mL=57,629.081 g
Given that gasoline is primarily octane.
Mass of octane burnt in the tank = M = 57,629.081 g
Moles of octane =
According to reaction, 2 moles of octane gives 16 moles of carbon-dioxide.
Then 505.1637 mol of octane will give:
of carbon-dioxide
Mass of 4,041.3100 mol of carbon-dioxide:
4,041.3100 mol × 44.01 g/mol = 177,858.05 g
Mass of carbon-dioxide produced in pounds = 391.28771 pounds
391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.