11.114 2.00 L of N,, at 25 °C and 1.08 atm, is mixed with 4.00 I of O2, at 25 °C and 0.118 atm, and the mixture is allowed to react. How much NO, in grams, is produced? (9.2, 9.3, 11.7, 11.8) N2(g) + O2(8) → 2NO(8)

(6.9: Similar to Example 6.15 & For Practice 6.15) Find the ratio of effusion rates of argon gas and chlorine gas. O 0.751 O 1.33 O 3.15 O 0.317

The major constituents of the atmosphere are nitrogen, N2, and oxygen, O2. Dry atmospheric air at a pressure of 1.000 atm has a partial pressure of N3 of 0.781 atm and a partial pressure of Og of 0.209 atm. At high temperatures, N2 and Oz react to produce nitrogen monoxide (nitric oxide), NO. N2(2) + O2 (9) = 2NO(9) Suppose a sample of dry air is raised to 2105°C in a hot flame and then rapidly cooled to fix the amount of NO formed. If K, for this reaction at this temperature is 2.3 x 10, how many grams of NO would be produced from 329.0 g of dry air?

9. If 15.0 liters of neon at 25.0 °C can expand to 45.0 liters, what must the new temperature be to maintain constant pressure? (5 points) 10. A gas occupies 900.0 mL at a temperature of 27.0 °C. What is the volume at 132.0 °C? (5 points)

3. A fixed quantity of gas at 23.0°C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the volume the gas will occupy if the temperature is increased to 145°C while the pressure is held constant. (14.5L) Sign out DELL 5 alt ctri

(Q23) A sample of an unknown gas is held at a pressure of 850 torr, a volume of 722 mL, and a temperature of 274 K. What will the temperature (in K) be if the pressure is decreased to 565 torr and the volume is decreased to 607 mL? (3 sf)

320 29. Determine what happens to each variable below (increases, decreases, no change) under the stated conditions. Assume that all other variables not specifically mentioned are constant values. (10.4) (a) What happens to the pressure when the volume decreases? (b) What happens to the volume when the temperature increases? (c) What happens to the pressure when the temperature decreases? (d) What happens to the pressure when the amount of gas decreases? 30. Determine what happens to each variable below (increases, decreases, no change) under the stated conditions. Assume that all other variables not specifically mentioned are constant values. (10.4) (a) What happens to the volume if the amount of gas doubles? (b) What happens to the temperature when the pressure decreases? (c) What happens to the temperature when the volume increases? 34. Calculate the missing variables in each experiment below using Boyle's law. (10.5) (a) P, = 1.67 atm, V1 = 3.77 L, P2 = 0.229 atm, V2 = ? (b) P1 =…

What volume of 1.0 M sulfuric acid solution is needed to produce 30.0 mL of hydrogen gas at 293 K? Multiply this stoichiometric volume by five (fivefold excess) and report the total volume of sulfuric acid solution needed in milliliters. Enter a number with three significant digits.   note: 6.7 is the incorrect answer

Fill in the blanks: (3.8) What volume (in mL) will 10.0 g of CO2 (g) Occupy at 27 °C and 2.00 atm? Atomic mass: C 12.01 O 16.00 Analysis (Given): T (CO2) = | K n mol (CO2) = %3D moL (3 sig fig) Answer: V (CO2) = mL %3D (3 sig fig)