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2g of gas X are introduced into an evacuated flask kept at 25oC. The pressure is found to be 1atm. If 3g of another gas ‘Y’ are added to same flask, the total pressure becomes 1.5 atm. Assuming that ideal behavior, the molecular mass ratio of Mx and My is:
Correct answer is '3'. Can you explain this answer?
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2g of gas X are introduced into an evacuated flask kept at 25oC. The p...
Is introduced into the same flask at the same temperature, the pressure will change depending on the properties of the two gases.
To determine the final pressure of the gas mixture, we need to know the molar mass and number of moles of each gas.
First, let's find the number of moles of gas X using the ideal gas law equation:
PV = nRT
Rearranging the equation:
n = PV / RT
Given:
P = 1 atm
V = unknown (since the flask is evacuated, we don't know the volume)
n = 2g / molar mass of X
R = 0.0821 L·atm/mol·K
T = 25°C = 298 K
Plugging in these values:
n = (1 atm)(V) / (0.0821 L·atm/mol·K)(298 K)
Now, let's find the number of moles of the other gas:
n2 = 3g / molar mass of the other gas
Once we have the number of moles of each gas, we can calculate the total number of moles:
n_total = n + n2
Finally, we can use the ideal gas law to find the final pressure:
P_total = (n_total)(R)(T) / V
Since we don't know the volume, we can't calculate the exact final pressure without additional information.
To determine the final pressure of the gas mixture, we need to know the molar mass and number of moles of each gas.
First, let's find the number of moles of gas X using the ideal gas law equation:
PV = nRT
Rearranging the equation:
n = PV / RT
Given:
P = 1 atm
V = unknown (since the flask is evacuated, we don't know the volume)
n = 2g / molar mass of X
R = 0.0821 L·atm/mol·K
T = 25°C = 298 K
Plugging in these values:
n = (1 atm)(V) / (0.0821 L·atm/mol·K)(298 K)
Now, let's find the number of moles of the other gas:
n2 = 3g / molar mass of the other gas
Once we have the number of moles of each gas, we can calculate the total number of moles:
n_total = n + n2
Finally, we can use the ideal gas law to find the final pressure:
P_total = (n_total)(R)(T) / V
Since we don't know the volume, we can't calculate the exact final pressure without additional information.
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2g of gas X are introduced into an evacuated flask kept at 25oC. The p...
Answer is Mx/My=0.33
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2g of gas X are introduced into an evacuated flask kept at 25oC. The pressure is found to be 1atm. If 3g of another gas ‘Y’ are added to same flask, the total pressure becomes 1.5 atm. Assuming that ideal behavior, the molecular mass ratio of Mx and My is:Correct answer is '3'. Can you explain this answer?
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2g of gas X are introduced into an evacuated flask kept at 25oC. The pressure is found to be 1atm. If 3g of another gas ‘Y’ are added to same flask, the total pressure becomes 1.5 atm. Assuming that ideal behavior, the molecular mass ratio of Mx and My is:Correct answer is '3'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about 2g of gas X are introduced into an evacuated flask kept at 25oC. The pressure is found to be 1atm. If 3g of another gas ‘Y’ are added to same flask, the total pressure becomes 1.5 atm. Assuming that ideal behavior, the molecular mass ratio of Mx and My is:Correct answer is '3'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 2g of gas X are introduced into an evacuated flask kept at 25oC. The pressure is found to be 1atm. If 3g of another gas ‘Y’ are added to same flask, the total pressure becomes 1.5 atm. Assuming that ideal behavior, the molecular mass ratio of Mx and My is:Correct answer is '3'. Can you explain this answer?.
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