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How much minimum volume of CO at stp is needed to react completely with 0.112L of ATM pressure and 127degreeCto give CO2?
To determine the minimum volume of carbon monoxide (CO) needed to react completely with a given volume of gas at specified conditions, we can use the ideal gas law. At standard temperature and pressure (STP: 0°C and 1 atm), 1 mole of any gas occupies 22.4 L. The reaction between CO and oxygen (O₂) to produce carbon dioxide (CO₂) is as follows: 2 CO + O₂ → 2 CO₂. Given 0.112 L of gas at 127°C and atmospheric pressure, we first need to convert this gas to equivalent moles at STP using the ideal gas law, then determine the stoichiometry of the reaction. However, since the initial conditions are not at STP, we would need to use the combined gas law to find the volume of CO needed at STP based on the reaction stoichiometry, which would typically require more information than provided for a complete calculation. In summary, without further details or data, it's not possible to provide an exact volume of CO needed to react with the specified gas volume.
How many liters of carbon monoxide gas are formed if 0.75 moles of carbon react completely with silicon dioxide (Assume this reaction occurs at STP.)?
To determine the volume of carbon monoxide gas formed from 0.75 moles of carbon reacting with silicon dioxide, we first need to consider the balanced chemical equation for the reaction, which typically is: ( C + SiO_2 \rightarrow CO + Si ). This indicates that 1 mole of carbon produces 1 mole of carbon monoxide. Therefore, 0.75 moles of carbon will produce 0.75 moles of carbon monoxide. At standard temperature and pressure (STP), 1 mole of gas occupies 22.4 liters, so 0.75 moles of carbon monoxide would occupy ( 0.75 \times 22.4 = 16.8 ) liters.
Is CO a gas?
Yes. CO is the poisonous gas carbon monoxide.At STP and in all environmental conditions, it is a gas.It is created by the incomplete combustion of some fuels, and can prevent oxygen from entering the bloodstream by binding with the hemoglobin. In moderate to high concentrations in the air, it can be seriously harmful or fatal.
What volume of oxygen at stp is required to affect the combustion of 11 liters of ethylene at degree c and 380 mm of hg pressure?
To determine the volume of oxygen required for the combustion of 11 liters of ethylene (C₂H₄) at standard temperature and pressure (STP), we first note that the balanced combustion reaction is: C₂H₄ + 3 O₂ → 2 CO₂ + 2 H₂O. This indicates that 1 mole of ethylene requires 3 moles of oxygen. Since 11 liters of ethylene corresponds to approximately 11 moles at STP, the oxygen needed would be 3 times that volume, resulting in 33 liters of oxygen at STP.
What would be the volume in liters OF 85.5 grams of carbon monoxide at?
To calculate the volume of 85.5 grams of carbon monoxide (CO) at a specific temperature and pressure, we first need to determine the number of moles of CO using its molar mass (approximately 28.01 g/mol). Dividing 85.5 grams by the molar mass gives about 3.05 moles of CO. Using the ideal gas law (PV=nRT), if we assume standard temperature and pressure (STP: 0°C and 1 atm), one mole occupies 22.4 liters, so 3.05 moles would occupy approximately 68.4 liters. However, for an accurate calculation, temperature and pressure conditions must be specified.
What is the density of CO gas if G occupies a volume of ml?
To calculate the density of carbon monoxide (CO) gas, you need to know its molar mass, which is approximately 28.01 g/mol. Density (ρ) can be calculated using the formula ρ = mass/volume. If you have the volume of CO gas in milliliters (ml), you can convert it to liters (1 ml = 0.001 L) and then use the ideal gas law or the molar volume at standard temperature and pressure (STP) to find the mass. Once you have the mass, divide it by the volume in liters to find the density in g/L.
What volume of carbon monoxide at STP is needed to produce 541 mL of carbon dioxide?
Using the ideal gas law - the volume of a gas is independent of it composition and is determined solely by the equation PV=nRT. As one mole of CO would produce one mole of CO2 it would take 541 mL of CO to produce 541 mL of CO2.
What is the volume of 3.5mol of CO2 gas at STP?
The volume of gas that 3.5 moles of oxygen occupy can be easily found using the relationship of PV=nRT where P is the pressure, V is the volume, n is the moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
What is the density of CO2 gas at STP?
The density of CO2 gas at standard temperature and pressure (STP) is approximately 1.977 g/L. This value is derived from the molar mass of carbon dioxide (44.01 g/mol) divided by the molar volume at STP (22.4 L/mol). The calculation is as follows: 44.01 g/mol / 22.4 L/mol = 1.977 g/L. This density value is useful in various applications, such as in gas laws and stoichiometry calculations.
What is density of CO gas if 0.196 g occupies a volume of 100ml?
The density of CO gas can be calculated using the formula: density = mass/volume. Given the mass of CO gas (0.196 g) and the volume it occupies (100 ml), we can convert the volume to liters (1 L = 1000 ml) and then calculate the density as 0.196 g / 0.1 L = 1.96 g/L. So, the density of CO gas is 1.96 g/L.
How many grams of iron (Fe) will be produced if you start with 3.65 liters of carbon monoxide gas (CO) at STP?
Not enough information to answer ! You can't make Iron from CO gas.
Is CO a gas?
Yes. CO is the poisonous gas carbon monoxide.At STP and in all environmental conditions, it is a gas.It is created by the incomplete combustion of some fuels, and can prevent oxygen from entering the bloodstream by binding with the hemoglobin. In moderate to high concentrations in the air, it can be seriously harmful or fatal.
What volume of oxygen at stp is required to affect the combustion of 11 liters of ethylene at degree c and 380 mm of hg pressure?
To determine the volume of oxygen required for the combustion of 11 liters of ethylene (C₂H₄) at standard temperature and pressure (STP), we first note that the balanced combustion reaction is: C₂H₄ + 3 O₂ → 2 CO₂ + 2 H₂O. This indicates that 1 mole of ethylene requires 3 moles of oxygen. Since 11 liters of ethylene corresponds to approximately 11 moles at STP, the oxygen needed would be 3 times that volume, resulting in 33 liters of oxygen at STP.
What volume would 20.0 g of CO occupy at a temperature of 25 degrees C and a pressure of 105 kPa?
To find the volume, we first need to calculate the number of moles of CO using its molar mass. Then we can use the ideal gas law equation: PV = nRT, where R is the gas constant and T is the temperature in Kelvin. After calculating the number of moles, we can determine the volume of CO.
How many liters of oxygen are necessary for the combustion of 277 g of carbon monoxide assuming that the reaction occurs at stp the balanced equation is 2 co plus o2 equals 2 co2?
2CO + O2 -> 2CO2 find moles O2 gas 277 grams carbon monoxide (1 mole CO/28.01 grams)(1 mole O2/2 mole CO) 4.9447 moles O2 Now, since I am lazy, I use PV = nRT V = nRT/P V = (4.9447 moles O2)(0.08206 L*atm/mol*K)(298.15 K)/(1 atm) V = 120.978 Liters of oxygen, or, in sigi figi; 121 Liters of oxygen needed for this combustion
If 1.00 kg of Fe2O3 completely reacts with CO the volume of CO2 released at STP will be?
There are several different possible reactions of Fe2O3 with CO, depending on temperature and ratio of reactants. The simplest is probably Fe2O3 + CO ==>2FeO + CO21.00 Kg x 1000 g/Kg x 1 mole Fe2O3/160 g = 6.25 moles Fe2O3 moles CO2 produced = 6.25 moles CO2 Volume CO2 at STP = 6.25 moles x 22.4 L/mole = 140 Liters
what is the density of CO GAS IF 0.196 g occupied a volume of 100 ml?
100ml = 1 dm3 0.196g = 196x10-6kg Density = mass/volume Density of CO = 196x10-6 / 1 = 196x10-6 kg/dm3
