When a milkshake is taken in through a straw at a pressure of 0.071 atm, the straw contains 5.0 mL of liquid. How much liquid is consumed at 0.092 atm?

The amount of liquid consumed at 0.092 atm is calculated to be 3.86mL.

The volume of a substance at a given pressure can be calculated using Boyle's law as follows:

P1V1 = P2V2

Where;

According to this question, when a milkshake is taken in through a straw at a pressure of 0.071 atm, the straw contains 5.0 mL of liquid. The volume of the liquid consumed at 0.092 atm is:

0.071 × 5 = 0.092 × V2

0.355 = 0.092V2

V2 = 0.355 ÷ 0.092

V2 = 3.86mL.

Therefore, the amount of liquid consumed at 0.092 atm is calculated to be 3.86mL.

Learn more about Boyle's law at: link

3.86 mL

Explanation:

we are given;

We are required to determine the new volume, V₂?

We are going to use Boyle's law;

According to Boyle's law, for a fixed mass of a gas, volume and pressure are inversely proportional, at constant temperature.

That is, P = kV

Therefore;

P₁V₁ = P₂V₂

Hence;

V₂ = P₁V₁ ÷ P₂

    = (0.071 atm × 5.0 mL) ÷ 0.092 atm

    = 3.859 mL

    = 3.86 mL

Thus, the amount of liquid consumed is 3.86 L

african americans demonstrated their newly found freedom by relocating often in search of relatives whom they had been separated from during slavery. others established schools to educate freed people and they built institutions such as churches and political organizations to advocate for their rights.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: