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velikii [3]
1 year ago
9

Which of the following measurements have four significant figures? Select all that apply. A.1,001g B.120.0mL C.0.0007cm D.5,000s

Chemistry
1 answer:
Wittaler [7]1 year ago
6 0

Answer:

The answer(s) will be A and B

Explanation:

Hope this helps and may God bless you<3

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3 years ago
How many moles of Ag+ ions are present in 10 ml of a 0.75 M AgNO3 solution?
lana66690 [7]

Answer:

b. 7.5 x 10^-3

Explanation:

To solve this problem we need to keep in mind the <em>definition of molarity</em>:

  • Molarity = moles of solute / liters of solution

With the above information in mind it is possible to calculate the moles of solute, given the volume (10 mL) and concentration (0.75 M) of the solution:

  • First we<u> convert 10 mL to L</u> ⇒ 10 mL / 1000 = 0.01 L

Then we <u>calculate the moles of AgNO₃</u>:

  • moles of solute = Molarity * Liters of solution
  • 0.01 L * 0.75 M = 7.5x10⁻³ mol AgNO₃

<em>One mole of AgNO₃ contains one mole of Ag⁺</em>, thus the number of Ag⁺ moles is also 7.5x10⁻³.

5 0
3 years ago
Which statement best explains why heating a liquid affects its viscosity?
Artyom0805 [142]

Answer:

A

Explanation:

took test I'm pretty sure and found respond else where

5 0
3 years ago
Read 2 more answers
Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 x 10
Olenka [21]

Answer:

7.12 × 10⁻³ M/s

Explanation:

Step 1: Write the balanced reaction

2 SO₂ + O₂ ⇒ 2 SO₃

Step 2: Establish the appropriate molar ratio

According to the balanced equation, the molar ratio of O₂ to SO₃ is 1:2.

Step 3: Calculate the rate of formation of SO₃

The rate of loss of O₂ is 3.56 × 10⁻³ mol O₂/L.s. The rate of formation of SO₃ is:

3.56 × 10⁻³ mol O₂/L.s. × 2 mol SO₃/1 mol O₂ = 7.12 × 10⁻³ mol SO₃/L.s

7 0
3 years ago
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