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If you have 5.5 L of gas at 25 C. What temperature is the gas at if we increase the volume to 7 L?
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If you have 17 moles of gas at a temperature of 67 degrees Celsius and a volume of 25 liters and a temperature of 300 K how many moles of as do you have?
17.....you said it in the question.
What is the volume occupied by 025 moles of chlorine gas?
This volume is 6,197 399 5 at 25 0C.
A tank filled with propane gas has a temperature of 275 K and a pressure of 25 ATM what happens to the temperature if the pressure is increased to 100 ATM?
The properties of an ideal gas are summed up in chemistry and physics in this neat equation: PV = kT This is saying that (pressure) multipled by (Volume) = (the constant 'k') times (Temperature) . Without getting into all the units and the details, in order to answer this question we only have to understand that when one side of the equation increases, the other side of the equation has to increase by the same multiplier. Increasing the pressure from 25 ATM to 100 ATM, the left side of the equation (PV) is multiplied by 4. (The volume of the tank 'V' remains constant.) If propane behaves like an ideal gas or close to it, then the right side must also multiply by 4, and the absolute temperature becomes 4 times as great. If the tank is perfectly insulated and none of the heat escapes, then the gas in it rises in temperature from 275 K to 1100 K.
Is lithium a solid liquid or gas at room temperature 25?
Solid
A 25 ml sample of gas in enclosed in a gas tight syringe at 22 degrees Celsius if the syringe is immersed in an ice bath at 0 degrees Celsius what is the new gas volume?
25 ml. The volume would not change. Now pressure on the other hand...
What will happen to the volume of one liter of air if you increase its temperature from 25 degrees celsius to body temperature?
nothing
What happens to the volume of a gas if its temperature is reduced by 25 percent?
Assuming pressure stays constant, the volume decreases by 25%. PV = nRT.
What woul happen to the volume of the 100L weather balloon if its temperature increases from 25 C TO 125 C while the external pressure remain constant?
The universal gas equation is PV = nRT (Pressure x Volume = Number of moles x Universal Gas Constant x Temperature in Kelvin/Rankin). So - if Pressure is constant, the number of moles is constant, but the temperature increases from 25C (298 K) to 125C (398K) - a 34% increase, a similar 34% increase in volume will occur.
What is the temperature of a 25 L sample of gas if its volume is 100 L at 285 K?
285 K?
If you have 17 moles of gas at a temperature of 67 degrees Celsius and a volume of 25 liters and a temperature of 300 K how many moles of as do you have?
17.....you said it in the question.
What volume is occupied by 2.0g He at 25 degrees celsius and 775 mmHg?
A fixed quantity of gas at a constant pressure exhibits a temperature of 27 degrees Celsius and occupies a volume of 10.0 L. Use Charles's law to calculate: the temperature of the gas in degrees Celsius in atmospheres if the volume is increased to 16.0 L
What temperature in degrees Fahrenheit would a fixed volume of gas need to be heated to in order to double its pressure if it starts out at 25 degrees Fahrenheit?
58 F
Is F a gas at room temperature?
Yes, fluorine is a gas at room temperature/25 degrees Celsius.
If a gas with a volume of 525ml at a temp of -25Celsius is heated to 175Celsius what us the new volume of the gas pressure and the number of the moles are held constant?
Assuming the gas follows the ideal gas law (which at these temperatures and pressures should be a good assumption), T2/T1 = P2V2/P1V1 so T2 (final temperature) = T1 x P2V2/P1V1 Temperature has to given in absolute temperature for this to work, so we first convert T1 25°C = 278.15 K. T2 = (278.15 K)(47.3 kPa)(7.0 L)/(95.3 kPa)/(2 L) = ~386.55 K = ~113.40 °C If it seems strange to you that the temperature went UP when the gas expanded, consider this... If the temperature remained constant, then as the pressure dropped to 47.3 kPa, the volume would only increase to about 5 L. To make the volume increase to 7 L at that pressure you would have to heat the gas up get it to expand.
How do you calculate the pressure of a gas in a cylinder with avolume of 15.0 L and filled with 50.0 g of gas at 25 degrees celsius?
50.0 grams of what gas? This is the ideal gas law. Pressure * Volume = moles gas * the R constant * temperature in Kelvin PV = nRT
When A balloon has a volume of 10500 liters and the temperature is 15 and degC. If the temperature were -25 and degC what would the volume of the balloon be?
It would be approx 9042 litres.
What is the volume occupied by 025 moles of chlorine gas?
This volume is 6,197 399 5 at 25 0C.
