Circle the true statement(s). If the statement is false, rewrite it to make it t
ID: 902393 • Letter: C
Question
Circle the true statement(s). If the statement is false, rewrite it to make it true. When 2.0 L of hydrogen gas are combined with 2.0 L of oxygen gas at 25degree C and 1.0 atm, 2H2(g) + 02(g) - 2H20(g) 4.0 L of steam are obtained. A gas at 25degree C in a 10.0 L sealed stainless steel tank has a pressure of 1.00 atm. When the temperature in the tank is doubled to 50 degree C, the volume of the tank doubles. the pressure in the tank doubles. the number of moles of gas doubles. the kinetic energy of the molecules increases. the velocity of the molecules stays the same. A tank has a total pressure of 1.00 atm. It contains 25.0 g of oxygen and 25.0 g of sulfur dioxide. The partial pressure of oxygen in the tank is 0.500 atm. What is the density of CO2 (g) at 745 mm Hg and 32 C? A gas has a density of 1.10 g/L at 27 C and 0.750 atm. What is its molar mass? Fifteen mL of HCI is added to aluminum metal producing 125 mL of hydrogen gas at 25degree C and 1.00 atm. What is the molarity of the HCI added? Consider two bulbs connected by a valve. Bulb A has a volume of 200.0 mL and contains nitrogen gas at a pressure of 0.500 atm. Bulb B has a volume of 1.00 L and contains CO gas at a pressure of 1.00 atm. What is the pressure in the two tanks when the valve is opened? The volume of the connecting tube and valve is negligible. Nitrogen does not react with carbon monoxide. CHALLENGE PROBLEM: What would the pressure in both tanks be if nitrogen were replaced by oxygen in bulb A under the same conditions?Explanation / Answer
Challenge problem.
let us consider T = 25 C
No of moles of N2 in Bulb A = PV/RT = 0.5*0.2/(0.0821*298)
= 0.00409 mole.
No of moles of CO in Bulb B = 1*1/(0.0821*298) = 0.0409 mole.
when valve is opened,
total volume = 1+0.2 = 1.2 L
total no of moles of mixer = 0.0409+0.00409 = 0.04499 mole
so that,
Pressure of mixer = 0.04499*(0.0821*298)/1.2 = 0.917 atm
if N2 in Bulb A is replaced by O2 .
No of moles of o2 in Bulb A = PV/RT = 0.5*0.2/(0.0821*298)
= 0.00409 mole.
2CO+O2 ---> 2co2
then
0.00409 mole of O2 reacts with 2*0.00409 mole of CO and gives
2*0.00409 mole of CO2.
therefore,
total no of moles of mixer = No of moles of CO mole.
total volume = 1+0.2 = 1.2 L
Pressure of mixer = 0.0409*(0.0821*298)/1.2 = 0.834 atm
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