From the stoichiometry of the problem, 2.01 × 10^5 g of zinc phosphate is produced.
<h3>What is volume?</h3>
Volume is the product of width, height and depth. The significant figures of the width, height and depth are 5, 4 and 6 respectively.The volume of the box is; 11.014 × 10^-2 m × 0.2481 m × 523.735 × 10^-3 = 0.01431 m^3 or 14310 cm^3 or 0.5053ft^3.
Density of zinc = 7.140 g / cm3
Volume of zinc = 14310 cm^3
Mass of zinc = 7.140 g / cm3 × 14310 cm^3 = 102 Kg
Moles of Zinc = mass /molar mass = 102 × 10^3/65 g/mol = 1569 moles
There are 195 g of zinc in 386 g zinc phosphate
102 × 10^3 g of Zn will produce x g
x = 102 × 10^3 g × 386 g / 195 g
x = 2.01 × 10^5 g of zinc phosphate
Learn more about stiochiometry: brainly.com/question/9743981
Answer:
15.9994 amu
Explanation:
By definition 1 mole of any substance is the mass that contains 1 Avogadro's Number of particle. (=> 6.02 x 10²³ particles/mole).
1 mole Oxy => 15.9994 amu => contains 6.02 x 10²³ particles Oxy /mole
1 mole Sulfur => 32.064 amu => contains 6.02 x 10²³ particles Sulfur /mole
1 mole H₂O => 18 amu => contains 6.02 x 10²³ molecules of water / mole.
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.
Answer:
The answer is B(scale)
Explanation:
Since the question asked about a range, the scale would be the most logical answer since scales are used to measure.
The answer is 2.0, and it is because
