Consider the following samples of gas: sample composition pressure temperature A 1.9 mol He (g) 1.8 atm 259. °C 1.9 mol He (g) 2.4 atm 299. °℃ 1.9 mol He (g) 1.5 atm 244. °C Select the set of graphs below that show the distributions of the speed of the atoms in each sample. B с number 2 speed 3 B 4 5 6 composition pressure temperature 3. °C 2.4 mol Kr (g) 1.2 atm 3.0 mol He (g) 1.2 atm 3. °C F 2.2 mol Ne (g) 1.2 atm 3. °C X sample D (Drag the slider to choose an image) 3 E 4 I 5 6

Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the CO₂ gas evolved by a certain chemical reaction taking place at 55.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 129. mL. g x10 177 Sketch of a gas-collection apparatus x collected gas Calculate the mass of CO₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. water chemical reaction

The compound Mg(ClO3)2 decomposes when heated according to the equation below. Mg(ClO3)2 (s) ➝ MgCl2 (s) + 3 O2 (g) An impure sample of material contains a small amount of Mg(ClO3)2 . The sample is heated and the gas produced collected by downward displacement of water. A total of 377.1 ml of gas is collected at a temperature of 20.0ºC when the atmospheric pressure is 740.0 torr. [The vapor pressure of water at 20.0ºC is 17.54 torr.]Calculate the number of grams of Mg(ClO3)2 present in the impure sample. Grams of Mg(ClO3)2 : Answer in grams

Constants | Periodic Table A gas of unknown molecular mass was allowed to effuse through a small opening under constant-pressure conditions. It required 105 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 29 s for 1.0 L of O2 gas to effuse. ▾ Part A Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.) Express your answer in grams per mol to two significant figures. M = Ο ΑΣΦ Submit Request Answer 3+ < Return to Assignment Provide Feedback a % ? g/mol MacBook Pro 曲 C

1) Consider the following reaction: Mg(s) + 2 HC1(aq) MgCl2 (aq) + H2(g) The total pressure of gas collected over water is 710.0 mmHg and the temperature is 23.0°C What is the pressure of hydrogen gas formed in mmHg? Pressure = mmHg

2.0 g of H2 gas and 4.0 g of He gas are contained in a 50.0-L gas-tight vessel 25.0o C. Calculate the partial pressure of each gas.

What is the partial pressure of O2 in the mixture?

A gas‑filled weather balloon has a volume of 56.0 L56.0 L at ground level, where the pressure is 761 mmHg761 mmHg and the temperature is 23.1 ∘C.23.1 ∘C. After being released, the balloon rises to an altitude where the temperature is −6.97 ∘C−6.97 ∘C and the pressure is 0.0772 atm.0.0772 atm. What is the weather balloon's volume at the higher altitude?

An unknown gas at 79.1 ∘C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior, what is the density of the gas? density:                                                g/L

A sample of gas contains 0.1700 mol of NH,(g) and 0.2125 mol of O,(g) and occupies a volume of 21.8 L. The following reaction takes place: 4NH3(g) + 502(g) 4NO(g) + 6H,O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.