# Problem: The density of a gas is 1.96 g/L at STP. What would the mass of 2.00 moles of the gas be at STP?1. 87.8 g2. There is not enough information to solve.3. 44.8 g4. 0.0875 g5. 43.9 g6. 0.510 g

🤓 Based on our data, we think this question is relevant for Professor Sparks' class at TEXAS.

###### FREE Expert Solution

We’re being asked to determine the mass of 2.00 moles of gas at standard temperature and pressure, given its density.

Recall that standard temperature and pressure (STP) is defined as 1 atm and 0 ˚C

The density of a gas is given by:

$\overline{){\mathbf{d}}{\mathbf{=}}\frac{\mathbf{PM}}{\mathbf{RT}}}$

where:

P = pressure (in atm)           R = gas constant (0.08206 atm • L/mol • K)

T = temperature (in K)         M = molar mass

d = density ###### Problem Details

The density of a gas is 1.96 g/L at STP. What would the mass of 2.00 moles of the gas be at STP?

1. 87.8 g

2. There is not enough information to solve.

3. 44.8 g

4. 0.0875 g

5. 43.9 g

6. 0.510 g

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Standard Temperature and Pressure concept. You can view video lessons to learn Standard Temperature and Pressure. Or if you need more Standard Temperature and Pressure practice, you can also practice Standard Temperature and Pressure practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofThe density of a gas is 1.96 g/L at STP. What would the mass...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 3 minutes and 33 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Sparks' class at TEXAS.