A sample of gas contains 0.2000 mol of CO(g) and 0.2000 mol of NO(g) and occupies a volume of 15.5 L. The following reaction takes place: 2CO(g) + 2NO(g) → 2CO2 (g) + N₂ (9) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = L

C3H4(g) + 4 O2(g) → 3 CO2(g) + 2 H2O(g) If 15.0 grams of C3H4(g) are placed in a 5.00L container at 350. K and allowed to react with CAcess O2(g) for 20 minutes, the partial pressure of CO2(g) is measured to be 4.50 atm. what mass of C3H4 will be left ? (Ideal gas law: PV = nRT, R= 0.082057 L atm/mole K) %3D %3D Complete the following table and use it to help you answer the question. -> 3 CO2(g) 2 H20(g) C3H4(g) 4 O2(g) initial moles change in moles new moles (expression) new moles (numerical value)

The International Space Station is equipped with a Vika Oxygen Generator which uses the following reaction to generate oxygen. LiClO4(s)→LiCl(s)+2O2(g) Determine the mass (in kg) of LiClO4 required to fill the 9.7 × 105 L interior volume of the International Space station with oxygen at a pressure of 0.21 atm and a temperature of 24.5 ˚C. You may find the following molecular weights useful: LiClO4 – 106.39 g/molLiCl – 42.394 g/molO2 – 31.9998 g/molReport your answer to accurate significant figures.

A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the storage unit rises to 76 °C, causing the gas to decompose and doubling the number of moles in the cylinder. Note: R = 0.08206 Latm/molK Determine the moles of gas in the cylinder before any decomposition occurs. Determine the pressure in the cylinder after the decomposition in atmospheres.

A sample of gas contains 0.1800 mol of CO(g) and 9.000×10-2 mol of O2(g) and occupies a volume of 12.4 L. The following reaction takes place:2CO(g) + O2(g)2CO2(g)Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

An ideal gas in a sealed container has an initial volume of 2.45 L.2.45 L. At constant pressure, it is cooled to 15.00 ∘C,15.00 ∘C, where its final volume is 1.75 L.1.75 L. What was the initial temperature?

A sample of gas contains 0.1100 mol of CH4(g) and 0.1100 mol of H2O(g) and occupies a volume of 7.46 L. The following reaction takes place:CH4(g) + H2O(g)3H2(g) + CO(g)Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. L

Consider the reaction N2(g) + 3H2(g) 2NH3 (g). What is the effect of decreasing the volume on the contained gases? The reaction shifts toward the product gas. O Ammonia is consumed in the reaction. O The system reacts by increasing the number of gas molecules. The pressure on the gases decreases momentarily. • Previous Nex acer

Consider the reaction below which was carried out at 200.0 K to produce liquid ammonia: N2(8) + 3H,(g) 2NH3() Suppose 37.3 g of N2 gas is mixed with 37.3 g of H2 gas. What is the volume (in units of liters) of gas remaining after the reaction is completed? The remaining gas was measured to have a temperature of 200.0 K and a pressure of 760.0 mmHg? molar mass of N2= 28.013 g/mol molar mass of H2 = 2.0158 g/mol. %3D Recall: Vo (1/P) (at constant Tand n) VaT (at constant P and n) Van (at constant Tand P) PV = nRT rate of effusion ox 1 atm 760 torr 760 mmHg %3D %3D R=8.31446 J K-1.r mol-1 R= 0.0820573L atm K-1. mol-1 %3D

A sample of gas contains 0.1800 mol of CO(g) and 0.1800 mol of NO(g) and occupies a volume of 16.0 L. The following reaction takes place: 2CO(g) + 2NO(g) → 2CO₂ (g) + N₂ (9) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = Submit Answer L Retry Entire Group 9 more group attempts remaining