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vampirchik [111]
2 years ago
13

A pharmacy technician measures the mass of a pill. the mass of one pill is 461 mg. what is the mass in kilograms of 100 pills? w

rite your answer as a decimal.
Chemistry
2 answers:
polet [3.4K]2 years ago
8 0
The mass of 100 pills is 461 x 100 = 46,100mg. 1 kilogram has 1000 grams and one gram has 1000 mg. so 46,100mg/1000=46.1 grams. So 46.1/1000=0.046kg for 100 pills. In other words, 46.1 grams / 1000 grams= 0.046 kg or <1/20th of a kg.
atroni [7]2 years ago
7 0

Answer:

The mass of 100 pills is 461 x 100 = 46,100mg. 1 kilogram has 1000 grams and one gram has 1000 mg. so 46,100mg/1000=46.1 grams. So 46.1/1000=0.046kg for 100 pills. In other words, 46.1 grams / 1000 grams= 0.046 kg or <1/20th of a kg.

Explanation:

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When one atom loses an electron and another atom accepts that electron a(n) bond between the two atoms results?
morpeh [17]
When an element losses its electron its called a cation. When an element accepted that electron it called anion. This is called an ionic bond.
8 0
2 years ago
Some household cleaners come in concentrations stronger than necessary for basic cleaning jobs. Jeremy followed the instructions
VashaNatasha [74]

Answer:

no he just repeated the steps and made more of the same cleaner my guy

Explanation:

5 0
2 years ago
A 20.0 -\,L volume of an ideal gas in a cylinder with a piston is at a pressure of 3.2 atm. Enough weight is suddenly removed fr
zzz [600]

Answer:

1. ΔE = 0 J

2. ΔH = 0 J

3. q = 3.2 × 10³ J

4. w = -3.2 × 10³ J

Explanation:

The change in the internal energy (ΔE) and the change in the enthalpy (ΔH) are functions of the temperature. If the temperature is constant, ΔE = 0 and ΔH = 0.

The gas initially occupies a volume V₁ = 20.0 L at P₁ = 3.2 atm. When the pressure changes to P₂ = 1.6 atm, we can find the volume V₂ using Boyle's law.

P₁ × V₁ = P₂ × V₂

3.2 atm × 20.0 L = 1.6 atm × V₂

V₂ = 40 L

The work (w) can be calculated using the following expression.

w = - P . ΔV

where,

P is the external pressure for which the process happened

ΔV is the change in the volume

w = -1.6 atm × (40L - 20.0L) = -32 atm.L × (101.325 J/1atm.L) = -3.2 × 10³ J

The change in the internal energy is:

ΔE = q + w

0 = q + w

q = - w = 3.2 × 10³ J

6 0
2 years ago
9) After lab, all of Darrel’s friends looked at his data and laughed and laughed. They told him that he was 30.8% too low in the
zaharov [31]
If he was 30.8% too low, it means that he was at 69.2% of the boiling point needed. So 50o C is 69.2% of total.

In order to know what 100% is, you can divide the number by it's percentage and then multiply it by a hundred.

So: 50/30.8=1.623
1.623*100=162.3
So the correct boiling point of the liquid he was working with in the lab is 162.3 oC
3 0
2 years ago
Read 2 more answers
During a lab experiment performed at STP conditions, you prepare HCl by reacting 100. ml of Cl2 gas with an excess of H2 gas.
Brrunno [24]

Answer: 19.4 mL Ba(OH)2

Explanation:

H2(g) + Cl2(g) --> 2HCl(aq) (make sure this equation is balanced first)

At STP, 1 mol gas = 22.4 L gas. Use this conversion factor to convert the 100. mL of Cl2 to moles.

0.100 L Cl2 • (1 mol / 22.4 L) = 0.00446 mol Cl2

Use the mole ratio of 2 mol HCl for every 1 mol Cl2 to find moles of HCl produced.

0.00446 mol Cl2 • (2 mol HCl / 1 mol Cl2) = 0.00892 mol HCl

HCl is a strong acid and Ba(OH)2 is a strong base so both will completely ionize to release H+ and OH- respectively. You need 0.00892 mol OH- to neutralize all of the HCl. Note that one mole of Ba(OH)2 contains 2 moles of OH-.

0.00892 mol OH- • (1 mol Ba(OH)2 / 2 mol OH-) • (1 L Ba(OH)2 / 0.230 M Ba(OH)2) = 0.0194 L = 19.4 mL Ba(OH)2

3 0
2 years ago
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