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A student calculates that the volume of his textbook is 991.880 cm3. what is the volume written with 3 significant figures?

k0ka [10]

The volume of the textbook calculated by the student written to 3 significant figures is 992cm³

According to this question, a student calculates the volume of his textbook and arrived at an answer of 991.880 cm³.

To round up this digit to 3 significant figures, which means that only 3 significant numbers should appear in the answer.

To do this, the number after the third number is 8, which means we can round up the value of 1 to 2. Hence, the volume of the textbook calculated by the student is 992cm³ in 3 s.f.

Learn more at: brainly.com/question/16563962?referrer=searchResults

7 0

3 years ago

You are planting flowers in large pots. You plan to plant flowers in 10 pots. 15 cups of potting soil will fill one pot. A bag o

dimaraw [331]

Answer:

I will need six (6) bags of potting soil

Explanation:

Since you plan on planting in 10 pots and need 15 cups of potting soil per pot, the total amount of potting soil you need <em>(in cups)</em> is 10 X 15 = 150 cups of potting soil.

We have that a bag contains 25 sups. to get the number of bags needed, we have to divide 150 by 25. This will give us 150 / 25 = 6 bags.

Therefore, I will need six (6) bags of potting soil

3 0

4 years ago

Calculate the solubility in g/l of lead (ii) fluoride in water at 25 oc if ksp of pbf2 is 4. 1 x 10-8.

Svetlanka [38]

The solubility of Lead(II)Fluoride is 2.17 × 10⁻³ g/L in water at 25°C.

At a specific solution temperature, a solid salt compound can entirely dissolve in pure water up to a predetermined molar solubility limit. The dissociation stoichiometry ensures that the molarities of the constituent ions are proportionate to one another. The saturable nature of the solution causes them to also coexist in a solubility equilibrium with the solid component. At this temperature, a solubility product constant Ksp is calculated using the solubility product of their molarity values.

Lead (II) fluoride has the following solubility equilibrium for its saturated solution:

$PbF_2(s)$ ⇄ $Pb^2^+ (aq) + 2F^- (aq)$

$K_s_p = [Pb^2^+][F^-]^2$

This compound dissociates in a 1:2 ratio of ions. For the compound dissolved in pure water, the Ksp is expressed in terms of the molar solubility "x" as:

$K_s_p = (x) (2x)^2\\$