2.4
4.005
To find the number of moles of oxygen in 0.16 g of oxygen gas, you first need to determine the molar mass of oxygen (O2), which is about 32 g/mol. Then, you can use the formula moles = mass / molar mass to calculate the number of moles. In this case, 0.16 g / 32 g/mol = 0.005 moles of oxygen gas.
To find the number of moles of ammonia gas, you can use the ideal gas law equation: PV = nRT. Convert the volume to liters (202mL = 0.202L) and the temperature to Kelvin (35°C + 273 = 308K). Plug in the values: (0.750 atm) * (0.202 L) = n * (0.0821 Latm/molK) * (308K), solve for n to find the number of moles of ammonia gas.
To find the number of moles of ammonia gas, first convert the volume to liters (202 mL = 0.202 L). Then use the ideal gas law (PV = nRT) to calculate the number of moles. Given that the temperature is 35°C (308 K) and the pressure is 750 mmHg (0.987 atm), you can rearrange the ideal gas law to solve for moles (n = PV/RT). Plugging in the values, n = (0.987 atm * 0.202 L) / (0.0821 L·atm/mol·K * 308 K) = 0.00851 moles of ammonia gas.
To calculate the number of moles of nitrogen gas in 35.7 g, you can use the molar mass of nitrogen, which is 28 g/mol. First, divide the given mass by the molar mass to find the number of moles: ( \frac{35.7 , \text{g}}{28 , \text{g/mol}} \approx 1.275 , \text{mol}). Therefore, there are approximately 1.275 moles of nitrogen gas in 35.7 g.
To find the mass of a gas, you need to know the volume of the gas, its pressure, temperature, and molar mass. Use the ideal gas law equation (PV = nRT) to calculate the number of moles of gas present. Then, multiply the number of moles by the molar mass of the gas to determine its mass.
You can find the number of moles using 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. Rearrange the equation to solve for n: n = PV / RT.
To find the number of moles of hydrogen gas, we first need to convert the mass of hydrogen gas from grams to moles using the molar mass of hydrogen gas (2 g/mol). 5.04 grams of hydrogen gas is equal to 5.04 g / 2 g/mol = 2.52 moles of hydrogen gas.
In the ideal gas law, n represents the number of moles of gas present in the system. It is a measure of the quantity of gas particles and is used to calculate the amount of gas based on the number of moles rather than individual particles.
If the number of moles of gas decreases, the volume of the gas will decrease as well, assuming constant temperature and pressure. This is described by Boyle's Law, which states that the volume of a gas is inversely proportional to the number of moles of gas when pressure and temperature are held constant.
You can use the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature. Rearrange the equation to solve for n (number of moles), and then use the molar mass of the gas in the cylinder to find the mass of the gas inside.
n is the number of moles.
If the number of moles of a gas doubles at constant pressure and temperature, the volume of the gas will also double according to Avogadro's law. This is because the volume of a gas is directly proportional to the number of moles present.
No
When the number of moles of a gas doubles and all else is constant, then the volume also doubles.
To find the number of moles of hydrogen gas, we first need to calculate the number of moles of chlorine gas using the ideal gas law formula (PV = nRT). Once we have the moles of chlorine gas, we can determine the moles of hydrogen gas needed for the reaction. In this case, the stoichiometry of the reaction states that 1 mole of chlorine gas reacts with 1 mole of hydrogen gas, so the required moles of hydrogen gas will be equal to the moles of chlorine gas.
4.005