A sample of helium gas occupies 12.9 L at 315 K and 1.20 atm.

Now, construct a balanced equation:



exists in its gaseous form as a diatomic molecule.

In the case of a 100m Race, displacement equals the distance traveled. If we divide this equation by the time t (assuming t represents the time taken to finish the 100m race), we derive that velocity equals speed. Conversely, in a 400m race where a full lap is completed, the racer’s starting and ending positions overlap, leading to displacement equaling 0, while the distance is not zero (400m). Therefore, it follows that displacement does not equal distance, leading to the conclusion that velocity does not equal speed.

Answer: 1.14

Explanation:

To find the molarity of the acid, we will utilize the equation derived from the neutralization process:

where

are the n-factor, molarity, and volume for the acid and

represent the n-factor, molarity, and volume for NaOH.

We know that:

By substituting the known values into the equation, we get:

To determine the pH of gastric juice:

The molarity amounts to = 0.072

Thus, the pH level of the gastric juice is 1.14

0.22 M

Answer:

0.400 moles of Oxygen

Explanation:

By employing the equation PV = nRT, the initial pressure of the flask can be calculated prior to the reaction, which leads to:

P = nRT/V

Where:

n signifies moles (4,000 moles: 2,000 moles of CO and 2,000 moles of H₂O)

R represents the gas constant (0.082 atm·L/mol·K)

T is the temperature (300.0 K)

V denotes volume (0.2000 L)

Substituting values results in P = 492.0 atm

To achieve a pressure reduction of 10.00%, the resulting pressure should be:

492.0 atm - 49.2 atm = 442.8 atm

Calculating with the new pressure under the same conditions gives the moles as:

n = PV/RT

n = 3,600 total moles

In the reaction:

2CO(g) + O₂(g) ⟶ 2CO₂(g)

The resulting moles are:

CO: 2,000 moles - 2X

O₂: 2,000 moles - X

CO₂: 2X

Where X accounts for the moles that react

Consequently, the total moles are:

4,000 moles - X = 3,600 moles

X = 0.400 moles

This indicates that the amount of oxygen needed for the reaction is 0.400 moles of Oxygen

I hope this is useful!