(Q33) What is the root mean square speed (UrMs) of fluorine gas at -60.3 °C?

What is the density of mustard gas, C4H8Cl2S, at 265 mmHg and a temperature of 315K

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1. A gas balloon has a volume of 106.0 liters when the temperature is 318.2 °K and the pressure is 740.0 mm of mercury. What will its volume be at 293.15 °K and 780.0 mm of mercury pressure?

1. A student following the procedure described in this module collected the following data: mass Mg, g 0.0243 initial syringe volume, mL 1.0 final syringe volume, mL 26.5 barometric pressure, torr 754 temperature, K 298 (a) calculate the gas law constant (b) What would be the volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298 K? Use the value for R found in part 1.

The following equation represents the .partial combustion of methane, CH4 2CH4(g) + 302(g) 2C0(g) + 4H2O(g); At constant temperature and pressure, what is the maximum volume of carbon monoxide that can be obtained from 6.62 x 102 L of methane and ?3.31 x 102 L of oxygen L 102 x 2.21 .a O L 102 x 9.93 .b O L 103 x 1.32.C O L 102 x 6.62 .d O L 10° x 2.32.e O الصفحة التالية

Hydrogen gas (H2) and nitrogen gas (N2) are combined through the Haber process to produce ammonia gas (NH3). This industrial process occurs at extremely high temperatures and pressures. If 11.1 L N2 are combined with excess hydrogen gas and the pressure and temperature are maintained at 233 atm and 500 °C throughout the reaction, how many grams of ammonia gas will be produced? 3H2(?)+N2(?)→2NH3(?)

1) A 0.075 g sample of calcium is reacted with excess hydrochloric acid and it produced 48.50 mL of gas that was collected over water. If the atmospheric pressure was 756 mmHg and the temperature was 22.0°C. How many moles of the gas were produced? What value would you calculate for the gas constant, R? Ca (s)+ 2 HC1 (aq) → CaCl2(aq)+ H2 (g)

A chemist wants to find the empirical formula and the molecular formula of a compound that contains only carbon, hydrogen, and nitrogen. Complete combustion of 35.0 g of the compound produced 41.1 g H2O. A 65.2 g sample of the compound was analyzed for nitrogen, giving 35.6 L N2 (g) at 740 torr and 25 ºC. The effusion rate of the compound as a gas was measured and found to be 38.2 ml/min. The effusion rate of argon gas under identical conditions in 58.0 ml/min. Find the empirical formula and the molecular formula of the compound.

Calcium carbide reacts with water to produce acetylene gas according to the following equation CaC3(s)+2H20 c,H,(g) Ca(OH)2(aq) The product gas, C,H2 is collected over water at a temperature of 25 °C and a pressure of 757 mm Hg. If the wet C,H, gas formed occupies a volume of 9.69 L the number of grams of C,H, fomed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C