For an ideal gas, calculate the following quantities.(a) The pressure of the gas if 0.135 mol occupies 207 mL at 25°C.  atm (b) The temperature (in kelvins) at which 0.0250 mol occupies 1.00 L at 0.583 atm.  K (c) The number of moles in 3.00 L at -7°C and 725 torr. Remember 1atm = 760 torr.  mol (d) The volume occupied by 4.72  10-3

For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point of -196. °℃. Suppose the temperature of a sample of nitrogen gas is raised from 27.0 °C to 57.0 °C, and at the same time the pressure is increased by 5.0%. Does the volume of the sample increase, decrease, or stay the same? increase decrease stays the same If you said the volume increases or decreases, calculate the percentage change in % the volume. Round your answer to the nearest percent. x10 X Ś

A flask contains 740 mmHg of nitrogen (N2) gas in a 4.00 L container at 25.0 °C. If 44.0 g of carbon dioxide (CO2) gas is added to this flask at constant volume and temperature without any loss of the nitrogen already inside, what is the final pressure (in atm) of the container? Assume both gases behave as ideal gases. Given: 1 atm =760 mmHg Enter the numerical value (no units), using 3 significant figures. Type your answer...

A mixture containing 2.21 g each of CH4(g), C,H4(g) and CAH10(g) is contained in a 1.50 L flask at a temperature of 25°C. (a) Calculate the partial pressure of each of the gases in the mixture. PCH atm atm %3D PCH0 atm (b) Calculate the total pressure of the mixture. atm

I Need answer question 2 using question 1 information  QUESTION 1: using the formula for the ideal gas law and the value for the gas constant of 0.08206 L.atm/k/mol, what is the volume (in L) of 7.96 grams of dry hydrogen at 28.3C and 766 torr ( i got this answer as 96.91 L) 、 QUESTION 2: the student obtains the following data by following an experimental procedure to this on. base on this data, what is the value of R in (L.ATM/MOLE/K) that would be calculated? report the result to fours sig fig (using 273.15k for temperature conversion) Pressure of dry h2 = 740.9, temperature = 23.0 degrees C, mass pf mg used =0.037, volume of H2 = 39.45 ET units, conversion factor=1.000 what is the value of R in (L.ATM/MOLE/K) that would be calculated?

What is the volume, in liters, of 4.00 molesmoles of methane gas, CH4CH4, at 17 ∘C∘ and 2.00 atm? Express your answer with the appropriate units.

If a gas remains at constant pressure while its volume increases from 0.25Liters to 500 mL when its temperature is 208K, what must have been its original temperature? Whose gas law is this?

For many purposes we can treat ammonia  NH3  as an ideal gas at temperatures above its boiling point of  −33.°C .   Suppose the temperature of a sample of ammonia gas is raised from  −14.0°C  to  −1.0°C , and at the same time the pressure is increased by  15.0% .       Does the volume of the sample increase, decrease, or stay the same?   increase decrease stays the same       If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent. %

A typical fluorescent light bulb contains argon gas and mercury vapor. (a) If the total gas pressure in a fluorescent light bulb is 307.4 Pa and the partial pressure of the argon gas is 306.1 Pa, what is the partial pressure of the mercury vapor?  Pa(b) If a 930.-mL fluorescent bulb contains 4121 µg of argon gas and 81 µg of mercury vapor, what is the total gas pressure in the fluorescent bulb at 310. K?  Pa

The pressure in atm, if 8.25 × 10 ^-2mole of an ideal gas occupies a volume of 255 ml at 115 deg C.