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If the system is at equilibrium what happens if you lower the pressure of the system?
If the system is at equilibrium and you lower the pressure, the system will shift to favor the side with more gas molecules to counteract the decrease in pressure. This shift helps maintain the equilibrium condition. Ultimately, the equilibrium position may change to favor the formation of more gas molecules.
What is the equation for nitrogen gas plus hydrogen gas under pressure and at high temperature?
The equation for the reaction between nitrogen gas (N2) and hydrogen gas (H2) under pressure and at high temperature is: N2(g) + 3H2(g) → 2NH3(g) This is the Haber process, which is used to produce ammonia industrially.
What is the pressure of 64.0 g of oxygen gas in a 1.50L container at -37C?
To find the pressure of the oxygen gas, we can use the ideal gas law: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. First, convert -37°C to Kelvin by adding 273.15 (235.15 K). Then calculate the number of moles of oxygen using the given mass (64.0 g) and the molar mass of oxygen (32 g/mol). Finally, substitute the values into the ideal gas law equation to find the pressure.
What is the density of Cl2 gas at STP?
what is the volume of a balloon containing 50.0 moles of O2 gas at a pressure of 15.0 atm at 28 degrees
What volume will 125 g of CO2 occupy?
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
If the system is at equilibrium what happens if you lower the pressure of the system?
If the system is at equilibrium and you lower the pressure, the system will shift to favor the side with more gas molecules to counteract the decrease in pressure. This shift helps maintain the equilibrium condition. Ultimately, the equilibrium position may change to favor the formation of more gas molecules.
In which reaction will decreasing the pressure cause more reactants to form?
If the reaction involves a decrease in the number of moles of gas molecules on the reactant side compared to the product side, then decreasing the pressure will favor the side with more moles of gas. This is because reducing the pressure will shift the equilibrium towards the side with a higher number of gas molecules to help restore the pressure.
What is the equation for nitrogen gas plus hydrogen gas under pressure and at high temperature?
The equation for the reaction between nitrogen gas (N2) and hydrogen gas (H2) under pressure and at high temperature is: N2(g) + 3H2(g) → 2NH3(g) This is the Haber process, which is used to produce ammonia industrially.
What is chlorine's density in grams per milliliter or g mL?
Chlorine is a gas. Its density depends on pressure, temperature and volume of the container.
What is the pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide 1.73 g of sulfur dioxide and 3.33 g of argon at 42 degrees Celsius?
To find the total pressure in the vessel, you need to calculate the partial pressures of each gas using the ideal gas law. First, calculate the moles of each gas using the given mass and molar mass of each gas. Then, use the partial pressure formula (P = nRT/V) to find the partial pressure of each gas. Finally, sum up the partial pressures to get the total pressure in the vessel.
What happens if you lower the pressure of the system The system below is at equilibrium. 2co(g) plus o2(g) 2co2(g)?
Lowering the pressure of the system will cause the reaction to shift towards the side with fewer gas molecules to increase the pressure. In this case, the reaction will shift to the right, producing more CO2 gas molecules until a new equilibrium is reached.
What is the density chlorine?
The density of chlorine at 0 0C and normal atmospheric pressure is 3.2 g/L.
What is the density of argon gas?
The density of argon gas at standard conditions (0°C and 1 atm pressure) is approximately 1.784 g/L.
What is the pressure of 64.0 g of oxygen gas in a 1.50L container at -37C?
To find the pressure of the oxygen gas, we can use the ideal gas law: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. First, convert -37°C to Kelvin by adding 273.15 (235.15 K). Then calculate the number of moles of oxygen using the given mass (64.0 g) and the molar mass of oxygen (32 g/mol). Finally, substitute the values into the ideal gas law equation to find the pressure.
What does the symbol g represent in a chemical equation?
The symbol (g) is gas (in a chemical reaction) or gram.
How do you calculate the pressure of a gas in a cylinder with avolume of 15.0 L and filled with 50.0 g of gas at 25 degrees celsius?
To calculate the pressure of a gas in the cylinder, you can use the ideal gas law equation: PV = nRT. First, convert 50.0 g of gas to moles using the molar mass of the gas. Then, plug in the given values for volume (15.0 L), temperature (25 degrees Celsius), the ideal gas constant (R = 0.0821 L·atm/mol·K), and the calculated moles of gas. Solve for pressure (P).
What is the density of Cl2 gas at STP?
what is the volume of a balloon containing 50.0 moles of O2 gas at a pressure of 15.0 atm at 28 degrees
