If a sample of oxygen gas, originally at 5.00 atm in 1.00 L, is heated in that container from 25.0°C to 175°C, what is the final pressure? A: 7.52 atm B: 0.714 atm C: 0.133 atm D: 35.0 atm
P1 = 5.0 atm
A: 7.52 atm
V1 = 1.0 L
T1 = 25 oC = 298.15 K
P2 = to be calculated
T2 = 175 oC = 448.15 K
Volume (V2) = constant = 1 L
So,
P1 / T1 = P2 / T2
final Pressure (P2) = (P1 / T1) x T2 = (5.0 atm / 298.15 K) x (448.15 K) = 7.52 atm
If a sample of oxygen gas, originally at 5.00 atm in 1.00 L, is heated in...
A quantity of N2 gas originally held at 3.80 atm pressure in a 1.00 L container at 26.0ºC is transferred to a 10.0 L container at 20.0ºC. A quantity of O2 gas originally at 4.75 atm and 26.0ºC in a 5.00 L container is added to the 10.0 L container already containing the N2. a) Draw a diagram outlining this experiment, labeling the various quantities. b) Calculate the total pressure in the new container. c) What is the mole fraction...
A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25 degrees C. One now finds that the gas pressure inside the container is 1.73 atm. what mass of mercury (II) oxide was originally placed into the container? my answer is 153 g.... please show work and explain
1. A sample of gas initially at 782 torr and 1.00 L was heated to final temperature of 405 K with a final volume and pressure of 0.850 L and 926 torr, respectively. What was the initial temperature in Kelvin? 2. 1.81 moles of a gas at 305 K is placed into a 15.1 L container. What is the pressure inside the container in atm?
Answer: 2.3. A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25°C. One now finds that the gas pressure inside the container is 1.73 atm. What mass of mercury(II)oxide was originally placed into the container? Answer:
1.00-mol sample of N2 gas at 20.09C and 5.00 atm is allowed to expand adiabatically and quasi- C. After it reaches a temperature of 20.09C, it is heated at constant volume until its pressure 72..A stati cally until its pressure equals 1.00 atm. It is then heated at constant pressure until its temperature is is again 5.00 (a) Construct a PV diagram showing each process in the cycle. (b) From your graph, determine the work done by the gas during...
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured
at 1.00 atm and 25.0 0 degrees * C , 60.1 kl of heat is released at
constant pressure. What is AH for this reaction? (R = 0.0821L * atm
/ (Kmol)) 2Pb(s)+O 2 (g) 2PbO(s) )
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm and 25.0°C. 60.1 kJ of heat is released at constant pressure. What is AH°...
The volume of a sample of gas measured at 35.0°C and 1.00 atm pressure is 3.00 L. What must the final temperature be in order for the gas to have a final volume of 4.00 L at 1.00 atm pressure? ALL CALCULATIONS MUST BE PROVIDED FOR FULL CREDIT - 42.0°C -226.3°C 137.7°C 46.7°C 26.3°C
Part A A 1.00-mol sample of an ideal diatomic gas, originally at 1.00 atm and 27°C, expands adiabatically to 1.85 times its initial volume. What are the final pressure for the gas? (Assume no molecular vibration.) 0 AM O O ? Pf= atm Submit Request Answer Part B What are the final temperature for the gas? Express your answer using two significant figures. 10 ADC 0 2 ? T;
How do I do 28-35
28. A sample of gas measures 5.00 liters at 1.00 atm. To change the volume to 3.50 liters at constant temperature, what pressure must be applied? 29. How many moles of by drogen (He) fill a weather balloon whose volume is 250 liters at a pressure of 0.50 atm with a temperature of-10.0 C? 30. What is the pressure of 3.50 moles of helium at -50.0'C in a rigid container whose volume is 25.0 liters?...
A 1.00 mole sample of an ideal monatomic gas, originally at a pressure of 1.00 atm, undergoes, undergoes a three-step process. (1) It is expanded adiabatically from T1 = 550 K, to T2 = 389 K; (2) it is compressed at constant pressure until the temperature reaches T3; (3) it then returns to its original temperature and pressure by a constant volume process. (a) Plot these processes on a PV diagram. (b) Determine T3. (c) Calculate the change in internal energy, the...