0
What else can I help you with?
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 is the density in g L of chlorine gas at 7.50 102 torr and 25.0ºC Molar mass of chlorine equals 70.9 g mol?
The density of a gas can be calculated using the ideal gas law equation: density = (PM) / (RT), where P is pressure, M is molar mass, R is the ideal gas constant, and T is temperature in Kelvin. First, convert pressure to atm (7.50*10^-2 atm), temperature to Kelvin (25+273 = 298 K), and the ideal gas constant R = 0.0821 L atm/mol K. Then, plug in the values and calculate. The density of chlorine gas at these conditions will be approximately 3.21 g/L.
Suppose two gases in a container have a total pressure of 1.20atm what is the pressure of gas B if the partial pressure of gas A is 0.75atm?
The pressure of gas B can be calculated by subtracting the partial pressure of gas A from the total pressure. Therefore, the pressure of gas B would be 1.20 atm - 0.75 atm = 0.45 atm.
Which gas is produced by power station?
Power stations typically produce carbon dioxide gas as a byproduct of burning fossil fuels like coal, oil, or natural gas. This greenhouse gas contributes to climate change when released into the atmosphere in large quantities.
Omar was recording his preliminary data before beginning an experiment on gas behavior The room temperature was 298K and atmospheric pressure was 1 ATM Omar used an acceptable abbreviation of thes?
Omar used the abbreviation "298 K" for the room temperature and "1 atm" for the atmospheric pressure, which are the standard abbreviations for Kelvin and atmosphere, respectively. These abbreviations are commonly used in scientific literature to denote temperature and pressure values.
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
What is a gas at 273k and 1 ATM at?
At 273K and 1 ATM, most gases typically exist in the gaseous state. However, the specific gas present will depend on the composition of the system.
What is the pressure in atmospheres exerted by a 0.500 mol sample of oxygen gas in a 10.0 L container at 298 K?
To find the pressure exerted by the gas, we can use the ideal gas law, ( PV = nRT ). Here, ( n = 0.500 ) mol, ( R = 0.0821 , \text{L} \cdot \text{atm} / (\text{mol} \cdot \text{K}) ), and ( T = 298 , \text{K} ). Plugging in the values, we get ( P = \frac{nRT}{V} = \frac{0.500 \times 0.0821 \times 298}{10.0} \approx 1.22 ) atm.
What state is oxygen at 298 K?
Oxygen is a gas at 298 K.
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
The gas pressure in an aerosol can is 1.8 ATM at 25oC If the gas is an ideal gas what pressure would develop in the can if it were heated to 475oC?
Using the ideal gas law (PV = nRT), we can calculate the new pressure of the gas in the aerosol can. Given that the initial pressure (P1) is 1.8 ATM and the initial temperature (T1) is 25°C, we can rearrange the formula to find the new pressure (P2) at 475°C. Since the volume (V), moles of gas (n), and gas constant (R) remain constant, we can solve for P2: P2 = (P1 * T2) / T1 = (1.8 ATM * 748 K) / 298 K ≈ 4.5 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?
A. An increase in pressure from 2 ATM to 3 ATM will result in a decrease in volume of gas. B. An increase in pressure from 3 ATM to 4 ATM will result in a decrease in volume of gas. C. A decrease in pressure from 4 ATM to 1 ATM will result in an increase in volume of gas. D. An increase in pressure from 1 ATM to 3 ATM will result in a decrease in volume of gas.
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
What is the total pressure of a gas mixture containing partial pressures of 0.23 ATM ATM and 0.89 ATM?
1.54 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
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
