A balloon with a volume of 1.50 L is at a pressure of 760 torr and a
Question:
A balloon with a volume of 1.50 L is at a pressure of 760 torr and a temperature of 30°C. If the pressure is increased to 2300 torr and the temperature is raised to 72°C, what is the new volume of the balloon? L
At a temperature of 70oC, a gas inside a 7.73 L metal canister has a pressure of 500 torr. If the temperature is decreased to 15oC (at constant volume), what is the new pressure of the gas? torr
A balloon with a volume of 4.02 L is at a pressure of 0.99 atm and a temperature of 8.0oC. If the pressure is increased to 4.0 atm and the temperature is raised to 28oC, what is the new volume of the balloon? L
A 554 mL metal can contains 2.62 × 10−2 mol of He at a temperature of 298 K. What is the pressure (in atm) inside the can? Is this pressure greater than or less than standard atmospheric pressure? Pressure = Entry field with atm A 230 mL flask contains He at a pressure of 760 torr and a temperature of 27°C. What mass of He is present? g He
A 670. mL flask contains N2 at a pressure of 0.75 atm and a temperature of 20°C. What mass of N2 is present? g N2 a. How many moles of Ar are present in a 2.8 L flask that has a pressure of 1.04 atm at a temperature of 23°C? mol Ar b. What is the mass of this Ar? g Ar
A mixture of gases contains 0.72 mol of N2, 0.39 mol of O2, and 0.26 mol of He. The partial pressures of each gas (in atm and in torr) in a 23 L cylinder at 342 K are given below.
PN2 0.878969739130 atm 668.8 torr
PO2 0.476108608696 atm 364.8 torr
PHe 0.317405739130 atm 243.2 torr
What are the partial pressures and the total pressure if 0.50 mol of CO2(g) is added?
partial pressure of N2 atm torr
partial pressure of O2 atm torr
partial pressure of He atm torr
partial pressure of CO2 atm torr
Total Pressure atm torr
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