What is the mass of carbon monoxide at STP?

What is the mass of carbon monoxide at STP?

Molar mass of CO = 12 + 16 = 28 g/mol. Therefore, 22.4 L ( 22400 cm3) is the volume of 28g CO at STP. 56 cm3 will be the volume of (28/22400) x 56 = 0.07 g of CO at STP.

What is the mass of 50cm3 of carbon monoxide at STP?

How many grams of CO will occupy 50 cc at STP= 28×50/22400= 0.0625g.

What is the volume at STP of 7.1 gram of chlorine?

The volume of 7.1 gram of chlorine at STP is 2.249568 L. Solution: In chemistry STP stands for “Standard Temperature and Pressure”.

How do you convert mass to liters?

To convert a gram measurement to a liter measurement, divide the weight by 1,000 times the density of the ingredient or material. Thus, the weight in liters is equal to the grams divided by 1,000 times the density of the ingredient or material.

How do you find volume at STP?

It can be written as: V = nRT/P. “P” is pressure, “V” is volume, n is the number of moles of a gas, “R” is the molar gas constant and “T” is temperature. Record the molar gas constant “R”. R = 8.314472 J/mole x K.

What is volume at STP?

Standard temperature and pressure (STP) are a useful set of benchmark conditions to compare other properties of gases. At STP, gases have a volume of 22.4 L per mole. The ideal gas law can be used to determine densities of gases.

What is the mass of 56 cm?

Rahul was told by his teacher to Calculate mass of the following : I. 0.5 mole of N2​ gas. II.

What is the volume at STP of 7.1 g of chlorine?

What volume will cl2 occupy at STP?

At STP, 1 mole of chlorine gas occupies 22.4 L.

What is the volume of the gas at STP?

This conversions relies on the fact that a mole of gas at STP has a volume of 22.4 L. It is important to note, however, that if the conditions of the gas are different this conversion will NOT work. Under those conditions you must use the ideal gas law to convert between moles and liters. Let’s try some problems.

How do you convert between moles and volume at STP?

To convert between moles and the volume of a gas at STP, we will use the factor label method discussed in the first unit. This conversions relies on the fact that a mole of gas at STP has a volume of 22.4 L. It is important to note, however, that if the conditions of the gas are different this conversion will NOT work.

What is the molar mass of helium gas at STP?

We can find the value for n by dividing the mass of helium gas by its molar mass: Now, we can just plug all of these values in and solve for V: Assuming that helium behaves as an ideal gas, we know that a mole of ideal gas occupies 22.4 litres at STP. The atomic weight of helium is 4 g/mol, so 6 g is 1.5 moles.