Suppose you have 1 atm of gas A and 1 atm of gas B. If A and B react to form C with a 1 A: 1 B: 2 C stoichiometry, what will the pressure of C equal?
A) .082 atm
B) 2.3 atm
C) 1 atm
D) 0.5 atm
1. If a gas occupies 2 L at 3 atm, how many liters will it occupy at 6 atm if the temperature is not changed? a)1L b)2L c)3L d)4L 2. IF A GAS OCCUPIES 2 L AT 273 °C, WHAT IS THE VOLUME AT 0 °C IF THE PRESSURE DOES NOT CHANGE? a)0.5 L b)1 L c)2 L d)4 L 3. If a gas occupies 5 L at 298 K, what temperature is needed to reduce the volume to 2 L...
b. Suppose you had a 39.5 g sample of N (o) at 125 atm and 620 *C. What would be volume of your N (a) sample? c. At what temperature would 33.0 mol of H.(g) occupy 28.0 L at 1.00 atm? d. You are given an 19.3 L of an unknown gas (that can be found in air in varying amounts). It has a pressure of 1.00 atm at 298 K. When you determine its mass, you find that you...
Suppose you have a fixed container containing 0.255 moles of a gas (the identity of the gas doesn't matter). If the container volume is 0.748 L, and the temperature is 301.15 K, what is the pressure in atm? (R=0.0821 L'atm/mol-K) O A.0.784 atm OB. 0.00842 atm O C.7.84 x 104 atm D.8.42 atm
Suppose you have 0.664 mol of an ideal gas in a 0.454 L container at 39.97 atm. a) What is the temperature of this gas? b) Sketch a pressure versus volume graph for this ideal gas, either using the graph paper on the next page or in a spreadsheet such as Excel. Have the graph go out to 4 L and 70 atm. Use at least 6 points to draw this curve. c) On the graph from part b, use...
Question 2 (0.5 marks) Hydrogen gas. H. and oxygen gas, O2, can be reacted to form liquid water. If 2.00 g hydrogen Ras and 17.20 g oxygen gas are reacted in a 1.500 L flask at 25.0 °C, calculate the total gas pressure (atm) in the flask at 25°C. The vapor pressure of water is 23.8 mm Hg. Stoichiometry is involved in this question. Total gas pressure:
Question 2 (0.5 marks) Hydrogen gas, H2, and oxygen gas, Oz, can be reacted to form liquid water. If 2.00 g hydrogen gas and 17.20 g oxygen gas are reacted in a 1.500 L flask at 25.0 °C, calculate the total gas pressure (atm) in the flask at 25 °C. The vapor pressure of water is 23.8 mm Hg. Stoichiometry is involved in this question. Total gas pressure:
1. You have a 25.0 mL sample of gas at 25 °C and 1.49 atm. The volume is changed to 0.0450 L while the temperature remains constant. What is the pressure, in mmHg, of this gas under these new conditions?
You have two flasks of equal volume. Flask A contains hydrogen gas (H2) at 0°C and 1 atm of pressure. Flask B contains CO2 gas at 25°C and 2 atm pressure. a) What is the ratio of the average kinetic energy per molecule of H2/CO2? b) What is the ratio of the average kinetic velocity of H2/CO2 molecules? c) What is the ratio of the number of molecules of CO2/H2? d) What is the mass ratio of CO2/H2?
Question 2 (0.5 marks) Hydrogen gas, H2, and oxygen gas, Oz, can be reacted to form liquid water. If 2.00 g hydrogen gas and 17.20 g oxygen gas are reacted in a 1.500 L flask at 25.0 °C, calculate the total gas pressure (atm) in the flask at 25 "C. The vapor pressure of water is 23.8 mm Hg. Stoichiometry is involved in this question.
7. (3) You have a mixture of gas that contains 0.24 atm CO2, 0.52 atm N2 and 0.85 atm 02 gas. What is the total pressure of this gas? What is the percent of each gas in the total mixture?