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Given that,
P1 =84.5 kPa =0.834 atm
V1 =215 cm3 =0.215 L
T1 23.5oC =296.5 K
P2 =1 atm
T2 =273 K
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- (a) What is the gauge pressure in a 25.0 cc car tire containing 3.60 mol of gas in a 30.0-L volume? (b) What will its gauge pressure be if you add 1.00 L of gas originally at atmospheric pressure and 25.0 ? Assume the temperature remains at 25.0 cc and the volume remains constant.85. A gas, while expanding under isobaric conditions, does 480 J ofwork. The pressure of the gas is 1.6 3 105 Pa, and its initial volume is 1.5 3 1023 m3. What is the fi nal volume of the gas?3 R.Calculate the AS (J/K), if Fini The temperature of 6 mole of an ideal gas is increased from 176 K to 750 K, and its given that C,=R the volume is constant. O a. 72.3 O b. 542.3 о с. 162.7 O d. 108.5
- dx 4 Q1 21 Quarter 3> Files > GAS LAW TEST 1.docx EST 1.docx W TEST 1.docx (29.1 KB) 5. A sample of gas has a volume of 215 cm3 at 23.5°C and 84.6 kPa. What volume will the gas occupy at STP? 6.) A sample of a gas has an initial volume of 250ml at 1790 mnm HAn ideal gas that occupies 1.2m^3 at a pressure of 1 x 105 Pa and a temperature of 27C is compressed to a volume of 0.6m^3 and heated to a temperature of 227C. What is the new pressure? a. 333.33 kPa b. 444.44 kPa c. 555.55 kPa d. 666.66 kPa2. If 150.00 mL of N2 gas was collected at 760 torr, what is the new volume of the gas when the pressure is compressed to 740 torr at the same temperature? 1. The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure of the gas if its volume is reduced to 10.0 at the same temperature.
- 1. Solving Ideal Gas Law Problems Directions: Use the ideal gas law, "PV-nRT", and the universal gas constant R =0.0821 L'atm to solve the following problems: K*mol If pressure is needed in kPa then convert by multiplying by 101.3kPa / latm to get R =8.31 kPa"L/(K*mole). Show your answers legibly, concisely, and completely. Use separate sheet of paper. if i contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, 1.4. what is the pressure inside the container?7. If I have an unknown quantity of gas held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many moles of a. 143.0mol gas do I have? d. 0.3457mol b. 0.01004mol C. 146.0mol 8. If I have 21 males of g3s held at a2. A balloon has a volume of 4.0 L when at sea level (1.0 atm) at a room temperature of 28°C What will be its volume when inflated with the same amount of gas at an elevation where the atmospheric pressure is 700 mm Hg at 28°C?
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