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298K and 1.0ATM is room temperature at sea level therefore any oxides that you might see in daily life would be present at this point. One of the most obvious would be Iron Oxide aka rust.
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Which gas is produced by power station?
Carbon dioxide, water, nitrogen oxides, sulfur oxides, ashes formed from the oxides of other elements.
How many nitrogen molecules are contained in 1.00 L of nitrogen gas at 1.00 ATM and 298 K how many nitrogen atoms?
You could solve this in two ways: using the ideal gas law (Van der Waals parameters optional), or by using the density. Since you specify a pressure and temperature (in kelvin), I will use the ideal gas law. Ideal gas law: PV=nRT P = pressure = 1.00 ATM V = volume = 1.00 L n = moles = what you're solving for R = gas constant = 0.0821 L*ATM/(mol*T) (T is absolute temperature (kelvin)) T = absolute temperature = 298 K (1.00atm)(1.00L) = n(0.0821L*ATM*mol-1T-1)(298K) n = 0.04 moles An = Avogadro's Number = number of molecules in one mole = 6.022141 * 1023 0.04 * 6.022141*1023 = 2.409 * 1022 molecules of N2 in 1.00L at 1.00atm and 298K
What volume would 32 g of NO2 gas occupy at 3.12 ATM and 18 Celsius?
(32.0 g/46.0 g/mol) (0.0821 atm) (291.0 K) / 3.12 atm
A vessel with an internal volume of 10.0L contains 2.80g of nitrogen gas 0.403g of hydrogen gas and 79.9g of argon gas At 25 degrees C what is the pressure in ATM inside the vessel show work?
5.62 atm
Which type of oxide is formed when metals combine with oxygen?
Metal oxides form alkalis when they dissolve in water. Non-metal oxides for acids. For example: carbon dioxide + water --> carbonic acid magnesium oxide + water --> magnesium hydroxide
A 150.0 ML sample of gas is collected at 1.20 ATM and 25 C what volume does the gas have at 1.50 ATM and 20.0 Ccould you show work?
PV/T=PV/T 1.20 ATM * 150.0 ML / 25 C = 1.50 ATM * V / 20.0 C 1.20 ATM * 150.0 ML / 298 K = 1.50 ATM * V / 293.2 K 1.20 ATM * 150.0 ML / 298 K / 1.50 ATM * 293.2 K = V 118 ML = V
0.783 g of hydrogen gas is placed in an container of volume 657 mL at a temperature of 342 K What is the pressure in ATM?
0.783 g of hydrogen gas is placed in an container of volume 657 mL at a temperature of 342 K. What is the pressure in atm?
A sample of a gas pressure of 3.00atm at 25c what would the gas pressure be at 52c if the volume remaiins constant?
25C is 298K. 52C is 325K. Assuming linearity (an ideal gas), P=3*325/298=3.27 atm.
According to the phase diagram for H2O what happens to the phases of water at 0 degC as the pressure is increased from 0 ATM to 10 ATM?
water changes from a gas to a solid to a liquid
A gas has a pressure of 1.26 ATM and occupies a volume of 7.40 L If the gas is compressed to a volume of 2.93 L what will its pressure be assuming constant temperature?
P1= 1.26 ATMV1= 7.60 LV2= 2.93 LP2= ?P1V1= P2V2.. . P2= 1.26 x 7.60 /2.93= 3.27 ATM
A cylinder contains 28.5 L of Oxygen Gas at a pressure of 1.8 ATM and a temperature of 298 K How much gas in mols is in the cylinder?
You must use the perfect gas law, which states that PV=nRTP= pressureV= volumen= number of molesR= universal gas constantT= temperaturerearranging the equation to solve for n we get n= PV/RTso n= 1.8(28.5)/8.314(298)n= 51.3/2477.572n= 0.021.09
Are inert gases and royal gases the same?
'Royal gas' is not a term used in chemistry. Perhaps you mean "noble gas", if so yes "inert gas" and "noble gas" often mean the same thing. However, oxides and fluorides of some of the "noble gasses " do exist, it might be best to think of them as "noble" rather than "inert". Xe, forms oxides.
Which gas is produced by power station?
Carbon dioxide, water, nitrogen oxides, sulfur oxides, ashes formed from the oxides of other elements.
What is the volume at stp of 720.0 ml of a gas collected at 20.0 c and 3.00 ATM pressure?
While STP is at 25oC (298 K) and 1 ATM, the ideal gas law (P1.V1 / T1 = P2.V2 / T2) states the following solution: [T2/T1]*[P1/P2]*V1 = V2[(273+25.0) K / (273+20.0) K] * [3.00 atm / 1.00 atm] * 720.0 mL =[298.0 / 293.0] * [3.00] * 720.0 = 2197 mL
If a mixture of two gases has a total pressure of 5.7 ATM. If one gas has a partial pressure of 4.1 ATM what is the partial pressure of the other gas?
1.6 ATM
What change in pressure would result in the volume of gas increasing A 2 ATM to 3 ATM B 3 ATM to 4 ATM C 4 ATM to 1 ATM D 1 ATM to 3 ATM?
Decreasing the pressure of a gas will increase its volume -- C
What is the total pressure of a gas mixture containing partial pressures of 0.23 ATM ATM and 0.89 ATM?
1.54 atm
