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MAXImum [283]
2 years ago
12

What is the energy of electromagnetic radiation with wavelength of 568 nm?

Chemistry
1 answer:
anygoal [31]2 years ago
6 0

Apr 15, 2020 · 1 answer
How to get unblocked. 1. See answer. Add answer. Log in to add comment. lunlun02015 is waiting for your help. Add your
You might be interested in
In a single displacement reaction between Sodium Phosphate and Barium, how much of each product (in grams) will be formed from 1
mixer [17]

Answer:

14.6 g of barium phosphate

3.35 g of sodium metal

Explanation:

2Na3PO4(aq) + 3Ba(s) -------> Ba3(PO4)2(aq) + 6Na(s)

The first step in any such reaction is to but down the balanced reaction equation according to the stoichiometry of the reaction.

The two products formed are barium phosphate and sodium metal.

Number of moles of barium corresponding to 10.0g of barium = mass of barium/ molar mass of barium

Molar mass of barium = 137.327 g

Number of moles of barium = 10/137.327

Number of moles of barium = 0.0728 moles

For barium phosphate;

3 moles of barium yields 1 mole of barium phosphate

0.0728 moles yields 0.0728 moles × 1/3 = 0.0243 moles of barium phosphate

Molar mass of barium phosphate = 601.93 g/mol

Therefore mass of barium phosphate = 0.0243 moles × 601.93 g/mol = 14.6 g of barium phosphate

For sodium metal

3 moles of barium yields 6 moles of sodium metal

0.0728 moles of barium yields 0.0728 × 6 / 3 = 0.1456 moles of sodium

Molar mass of sodium metal= 23 gmol-1

Mass of sodium metal= 0.1456g × 23 gmol-1 = 3.35 g of sodium metal

4 0
3 years ago
If 0.100 moles of AgNO₃ react with 0.155 moles of H₂SO₄ according to this UNBALANCED equation below, what is the mass in grams o
AlekseyPX

Answer:

15.6g Ag2SO4

Explanation:

2AgNO3 + H2SO4 --> Ag2SO4 + 2HNO3

-2x              -x

0.1-2x.       0.155-x

x=0.05      x=0.155

0.05mol Ag2SO4 x 311.78g = 15.6g Ag2SO4

4 0
3 years ago
Which of the following mixtures will react the fastest?
olga2289 [7]

Answer:

I think the answer would be A.

8 0
2 years ago
An unknown compound contains 38.7 % calcium, 19.9 % phosphorus and 41.2 % oxygen. what is the empirical formula of this compound
Softa [21]

Answer: Ca3(PO4)2

Explanation:

  • We assume that the sample is 100.0 g.
  • The sample contains 38.7 g of Ca, 19.9 g of P, and 41.2 g of O as the proportions show.
  • Then we can calculate the number of moles of each component (n = m/atomic mass).
  • The number of moles of Ca = 38.7/40.078 = 0.96 mol.
  • The number of moles of P = 19.9/30.97 = 0.64 mol.
  • The number of moles of O = 41.2/15.99 = 2.75 mol.
  • Now, we can get the molar ratios of different components (Ca, P, and O) in the sample by dividing the number of moles of each component by the lower number of moles, that we should divide the number of moles by (0.64).
  • Ca: P: O = (0.96/0.64) : (0.64/0.64) : (2.75/0.64) = 1.5 : 1 : 4.
  • To avoid the fraction of the ratios, we can multiply all ratios by 2.0.
  • Now, the ratio of Ca : P : O will be 3 : 2 : 8.
  • That main the empirical formula of the compound is Ca3P2O8 which can be expressed as calcium phosphate (Ca3(PO4)2).
8 0
2 years ago
Given that there are 6.02×1023 particles in 1.00 mole, how many h2o molecules are in 0.17 mole h2o?
Marizza181 [45]
1 mol ------------ 6,02×10²³
0,17 mol ------- X
X =(0,17×6,02×10²³)/1
X = 1,0234×10²³ molecules H₂O

:•)
6 0
3 years ago
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